A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction. I 2 ( a q ) + C l − ( a q ) → Concept introduction: There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants. The concept of writing a balanced chemical reaction is depends on conversion of reactants into products. First write the reaction from the given information. Then count the number of atoms of each element in reactants as well as products. Finally obtained values could place it as coefficients of reactants as well as products. Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced. Oxidation reduction and reduction reaction occur simultaneously in same reaction.

Question

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Answer 1

Question

Chapter 21, Problem 21.61QP

(a)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

I2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(a)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

I2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Iodine, in presence of Chloride ion is not a strong oxidizing agent that it doesn’t react with chloride ion.

(b)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Cl2(aq)+Br−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(b)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Chlorine, in presence of Bromide ion is a strong reducing agent that it reduces bromide ion to bromine.

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

(c)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+I−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(c)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Iodide ion is a strong reducing agent that it reduces iodide ion to iodine.

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

(d)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(d)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Chloride ion is not a strong reducing agent that it reduce chloride ion to chlorine.

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Answer 2

Question

Chapter 21, Problem 21.61QP

(a)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

I2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(a)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

I2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Iodine, in presence of Chloride ion is not a strong oxidizing agent that it doesn’t react with chloride ion.

(b)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Cl2(aq)+Br−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(b)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Chlorine, in presence of Bromide ion is a strong reducing agent that it reduces bromide ion to bromine.

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

(c)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+I−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(c)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Iodide ion is a strong reducing agent that it reduces iodide ion to iodine.

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

(d)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(d)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Chloride ion is not a strong reducing agent that it reduce chloride ion to chlorine.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 3

Question

Chapter 21, Problem 21.61QP

(a)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

I2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(a)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

I2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Iodine, in presence of Chloride ion is not a strong oxidizing agent that it doesn’t react with chloride ion.

(b)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Cl2(aq)+Br−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(b)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Chlorine, in presence of Bromide ion is a strong reducing agent that it reduces bromide ion to bromine.

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

(c)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+I−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(c)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Iodide ion is a strong reducing agent that it reduces iodide ion to iodine.

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

(d)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(d)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Chloride ion is not a strong reducing agent that it reduce chloride ion to chlorine.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 4

Question

Chapter 21, Problem 21.61QP

(a)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

I2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(a)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

I2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Iodine, in presence of Chloride ion is not a strong oxidizing agent that it doesn’t react with chloride ion.

(b)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Cl2(aq)+Br−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(b)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Chlorine, in presence of Bromide ion is a strong reducing agent that it reduces bromide ion to bromine.

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

(c)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+I−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(c)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Iodide ion is a strong reducing agent that it reduces iodide ion to iodine.

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

(d)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(d)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Chloride ion is not a strong reducing agent that it reduce chloride ion to chlorine.

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Subscribe now to access step-by-step solutions to millions of textbook problems written by subject matter experts!

Answer 5

Chapter 21, Problem 21.61QP

(a)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

I2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(a)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

I2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Iodine, in presence of Chloride ion is not a strong oxidizing agent that it doesn’t react with chloride ion.

(b)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Cl2(aq)+Br−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(b)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Chlorine, in presence of Bromide ion is a strong reducing agent that it reduces bromide ion to bromine.

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

(c)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+I−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(c)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Iodide ion is a strong reducing agent that it reduces iodide ion to iodine.

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

(d)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(d)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Chloride ion is not a strong reducing agent that it reduce chloride ion to chlorine.

Answer 6

Chapter 21, Problem 21.61QP

(a)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

I2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(a)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

I2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Iodine, in presence of Chloride ion is not a strong oxidizing agent that it doesn’t react with chloride ion.

Answer 7

Chapter 21, Problem 21.61QP

(a)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

I2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

Answer 8

(a)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

I2(aq)+Cl−(aq)→NR

Answer 9

(a)

Expert Solution

Answer 10

(a)

Expert Solution

Answer 11

Expert Solution

Answer 12

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Iodine, in presence of Chloride ion is not a strong oxidizing agent that it doesn’t react with chloride ion.

Answer 13

(b)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Cl2(aq)+Br−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(b)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Chlorine, in presence of Bromide ion is a strong reducing agent that it reduces bromide ion to bromine.

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Answer 14

(b)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Cl2(aq)+Br−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

Answer 15

(b)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Answer 16

(b)

Expert Solution

Answer 17

(b)

Expert Solution

Answer 18

Expert Solution

Answer 19

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Chlorine, in presence of Bromide ion is a strong reducing agent that it reduces bromide ion to bromine.

The balanced equation for the given reaction is,

Cl2(aq)+2Br−(aq)→Br2(aq)+2Cl−(aq)

Answer 20

(c)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+I−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(c)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Iodide ion is a strong reducing agent that it reduces iodide ion to iodine.

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Answer 21

(c)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+I−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

Answer 22

(c)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Answer 23

(c)

Expert Solution

Answer 24

(c)

Expert Solution

Answer 25

Expert Solution

Answer 26

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Iodide ion is a strong reducing agent that it reduces iodide ion to iodine.

The balanced equation for the given reaction is,

Br2(aq)+2I−(aq)→I2(aq)+2Br−(aq)

Answer 27

(d)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

(d)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+Cl−(aq)→NR

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Chloride ion is not a strong reducing agent that it reduce chloride ion to chlorine.

Answer 28

(d)

Interpretation Introduction

Interpretation:

A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.

Br2(aq)+Cl−(aq)→

Concept introduction:

There is a Law for conversion of mass in a chemical reaction i.e., the mass of total amount of the product should be equal to the total mass of the reactants.

The concept of writing a balanced chemical reaction is depends on conversion of reactants into products.

First write the reaction from the given information.

Then count the number of atoms of each element in reactants as well as products.

Finally obtained values could place it as coefficients of reactants as well as products.

Loss of electron and loss of Hydrogen in a compound is oxidation - the compound is oxidized. Gain of electron, gain of Oxygen in a compound is reduction - the compound is reduced.

Oxidation reduction and reduction reaction occur simultaneously in same reaction.

Answer 29

(d)

Expert Solution

Answer to Problem 21.61QP

The balanced equation for the given reaction is,

Br2(aq)+Cl−(aq)→NR

Answer 30

(d)

Expert Solution

Answer 31

(d)

Expert Solution

Answer 32

Expert Solution

Answer 33

Explanation of Solution

Halide ions and Halogens act as oxidizing and reducing agents. Reaction between halide ions and halogens depend upon their strength as oxidizing and reducing agent. A reducing agent loses electron whereas an oxidizing agent gains electrons.

A halide ion or halogen which is stronger oxidizing agent reacts only with a halide ion or halogen which is stronger reducing agent. Bromine, in presence of Chloride ion is not a strong reducing agent that it reduce chloride ion to chlorine.