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(a)
Interpretation:
A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.
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)
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Answer to Problem 21.61QP
The balanced equation for the given reaction is,
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:
A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.
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)
![Check Mark](/static/check-mark.png)
Answer to Problem 21.61QP
The balanced equation for the given reaction is,
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,
(c)
Interpretation:
A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.
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)
![Check Mark](/static/check-mark.png)
Answer to Problem 21.61QP
The balanced equation for the given reaction is,
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,
(d)
Interpretation:
A complete and balanced equation for the following reaction has to be written. ‘NR’ has to be written in case of no reaction.
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)
![Check Mark](/static/check-mark.png)
Answer to Problem 21.61QP
The balanced equation for the given reaction is,
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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Chapter 21 Solutions
General Chemistry - Standalone book (MindTap Course List)
- Write balanced net ionic equations for the following reactions in acid solution. (a) Liquid hydrazine reacts with an aqueous solution of sodium bromate. Nitrogen gas and bromide ions are formed. (b) Solid phosphorus (P4) reacts with an aqueous solution of nitrate to form nitrogen oxide gas and dihydrogen phosphate (H2PO4-) ions. (c) Aqueous solutions of potassium sulfite and potassium permanganate react. Sulfate and manganese(II) ions are formed.arrow_forwardFollow the directions of Question 23 for the following species: Cu+ Zn Ni2+ Fe2+ H+ (acidic)arrow_forwardOne of the few industrial-scale processes that produce organic compounds electrochemically is used by the Monsanto Company to produce1,4-dicyanobutane. The reduction reaction is 2CH2CHCH+2H++2eNC(CH2)4CN The NC(CH2)4CN is then chemically reduced using hydrogen gas to H2N(CH2)6NH2, which is used in the production of nylon. What current must be used to produce 150.kg NC(CH2)4CN per hour?arrow_forward
- (a) Write equations for the half-reactions that occur at the cathode and the anode when an aqueous solution of KCl is electrolyzed. Which chemical species is oxidized, and which chemical species is reduced in this reaction? (b) Predict the products formed when an aqueous solution of CsI is electrolyzed.arrow_forward1. If you wish to convert 0.0100 mol of Au3+ (aq) ions into Au(s) in a “gold-plating” process, how long must you electrolyze a solution if the current passing through the circuit is 2.00 amps? 483 seconds 4.83 104 seconds 965 seconds 1450 secondsarrow_forwardThree reactions very important to the semiconductor industry are The reduction of silicon dioxide to crude silicon, SiO2(s) + 2 C(s) → Si(s) + 2 CO(g) ΔrH° = 689.9 kJ/mol The formation of silicon tetrachloride from crude silicon, Si(s) + 2 Cl2(g) → SiCl4(g) ΔrH° = −657.01 kJ/mol The reduction of silicon tetrachloride to pure silicon with magnesium, SiCl4(g) + 2 Mg(s) → 2 MgCl2(s) + Si(s) ΔrH° = −625.6 kJ/mol Calculate the overall enthalpy change when 1.00 mol sand, SiO2, changes into very pure silicon by this series of reactions.arrow_forward
- An electrode is prepared from liquid mercury in contact with a saturated solution of mercury(I) chloride, Hg2Cl, containing 1.00 M Cl . The cell potential of the voltaic cell constructed by connecting this electrode as the cathode to the standard hydrogen half-cell as the anode is 0.268 V. What is the solubility product of mercury(I) chloride?arrow_forwardOrder the following oxidizing agents by increasing strength under standard-state conditions: O2(g); MnO4(aq); NO3 (aq) (in acidic solution ).arrow_forwardCalcium metal can be obtained by the direct electrolysis of molten CaCl2, at a voltage of 3.2 V. (a) How many joules of electrical energy are required to obtain 12.0 1b of calcium? (b) What is the cost of the electrical energy obtained in (a) if electrical energy is sold at the rate of nine cents per kilowatt hour?arrow_forward
- Using Table 17.1, calculate E° for the reaction between (a) chromium(II) ions and tin(IV) ions to produce chromium(III) ions and tin(II) ions. (b) manganese(II) ions and hydrogen peroxide to produce solid manganese dioxide (MnO2)arrow_forwardGiven HFH+(aq)+F(aq)Ka=6.9104HF(aq)+F(aq)H2(aq)K=2.7 calculate K for the reaction 2HF(aq)H+(aq)+HF2(aq)arrow_forwardBalance each of the following reactions, and identify the type of reaction CrCl3 (aq) + H2S(g) → Cr2S3(s) + HCl(aq)arrow_forward
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