4. For the following reactions: Balance each equation using half-reactions in the given conditions, and find the reduced and Oxidized reactants. a. Al + NO3→→ Al(OH)4 + NH3 (basic conditions) b. Zn(s) + NO3¯ (aq) – Zn+²(aq) + NH4+(aq) (acidic conditions) C. PbO2 (s) + 12(s) → Pb²+ (aq) +1O3- (aq) (acidic conditions) d. MnO4 + Sn(OH)4²→→ Sn(OH)6 ²- + MnO₂ (basic conditions) e. CN- (aq) + CrO4)²(aq) →CNO- (aq) + Cr(OH)3 (s) (basic conditions)

4. For the following reactions: Balance each equation using half-reactions in the given conditions, and find the reduced and Oxidized reactants. a. Al + NO3→→ Al(OH)4 + NH3 (basic conditions) b. Zn(s) + NO3¯ (aq) – Zn+²(aq) + NH4+(aq) (acidic conditions) C. PbO2 (s) + 12(s) → Pb²+ (aq) +1O3- (aq) (acidic conditions) d. MnO4 + Sn(OH)4²→→ Sn(OH)6 ²- + MnO₂ (basic conditions) e. CN- (aq) + CrO4)²(aq) →CNO- (aq) + Cr(OH)3 (s) (basic conditions)

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

See similar textbooks

Related questions

Q: When the following skeletal equation is balanced under acidic conditions, what are the coefficients…

Q: Balance the following reaction in basic solution. Fill in the coefficients for the balanced overall…

A: Redox reactions are the reaction in which one substance is getting oxidised and other getting…

Q: Balance the following oxidation-reduction reactions that occur in acidic solution using the…

A: Answer:- This question is answered by using the simple concept of balancing the redox reaction using…

Q: Balance with the half-reaction method in a basic, aqueous environment: CrO2(s) + NaClO (aq) → K¿CrO,…

Q: 9. Predict whether Co2* can oxidize Cl to Cl2 under standard state conditions. Explain your answer…

A: The reduction and oxidation reaction can be considered on the basis of the reduction potential of…

Q: Balance redox reactions in basic solution. Balance the reaction between F and HgO to form Hg and F2…

A: The given unbalanced redox reaction is: F-+HgO→Hg+F2

Q: lance each redox reaction. Label the half reactions as oxidation or reduction and identify the…

A: Balanced redox reaction:

Q: (1) Identify each of the following half-reactions as either an oxidation half-reaction or a…

A: The increase in oxidation no is oxidation & the decrease in oxidation no. Is reduction.

Q: Balance the following oxidation-reduction reactions that occur in basic solution. (Use the lowest…

A: To solve this problem, we have to balance the given chemical equations

Q: Zn(s) + Mno (s) Zn Zn2+(aq) + Mn 0 + Mn_0_(s) Write balanced oxidation and reduction half- reaction…

A: In a redox reaction, one species is oxidized (loses electrons) and another species is reduced (gains…

Q: Balance the following half-reactions by adding the appropriate number of electrons (e–). Then,…

Q: Consider the following unbalanced redox reaction. • Part A Cr203 (aq) + Cu (s) → Cr³+(ag) + Cu²+(aq)…

A: In a balanced chemical equation, the atoms of elements on both sides of the equation must be equal.

Q: 3. Complete and balance the chemical reaction using method of half-reactions. Write your answer in…

Q: f. CO₂(g) + Ca(OH)₂(aq) Ca(OH)₂(aq) →→→ CaCO3(s) + H₂O(aq) Oxidation numbers Atom oxidized Oxidizing…

A: we have to determine the oxidation states atom reduced atom oxidized reducing agent oxidizing…

Q: Identify the oxidizing and reducing agents in the following reaction. 3 Zn(s) + 2 CoCl3(aq)…

A: Lose of electrons is called oxidation And gain of electrons is called reduction. Species which get…

Q: VIII. Identify which element is oxidized and which is reduced. Write the half reactions for the…

A: An Oxidation -reduction reaction is any chemical reaction in which the oxidation number of Molecule…

Q: Substances A, B, and C can all act as oxidizing agents. In solution, A is green, B is yellow, and C…

A: Given : A , B and C all are oxidising agents and reduces to A- , B- and C- respectively. In…

Q: Balance the net ionic redox equations by the half-reaction method, both in acid and in base:…

A: While balancing redox reactions in acidic medium, we use H+(aq) ions and H2O(l) to balance H and O.…

Q: 39. Sketch a voltaic cell for each redox reaction. Label the anode and cathode and indicate the…

Q: 12. 13. Use the relative strengths of nonmetals and metals as oxidizing and reducing agents, as…

A: The objective of the question is to write the half-reactions.

Q: ) Identify each of the following half-reactions as either an oxidation half-reaction or a reduction…

A: SRp values for Sn is ESn+2/Sno = - 0.14 V Ag is EAg+1/Ag o = +…

Q: Give detailed Solution with explanation needed..don't give Handwritten answer..don't use Ai for…

A: Redox reaction is a reaction in which both oxidation and reduction reaction occur together.We have…

Q: 1. What must be added to the following half-reaction for it to be balanced? 10H^+ + NO3- (aq) +…

A: A redox reaction is balanced by balancing the mass and charge. Hence the number of atoms of all the…

Q: In the rusting of iron, the reduction reaction that occurs is: O Fe → Fe²+ + 2e™ Ⓒ2H₂O → O₂ + 4H* +…

A: Rusting of iron: The rusting of iron is a chemical reaction in which reddish brown coating forms on…

Q: You are asked to balance the following redox equation. What characteristics does this equation have…

A: The reaction given : We will balance this equation by half reaction methode due to the reason that…

Q: Hi, Balance each redox reaction using the half-reaction method, Mg(s) + Cr3+(aq) -----> Mg2+(aq)…

A: From the change in oxidation states the above reaction is divided into two half equations.

Q: Write the half reaction for the reduction part of this reaction. Cr,0? (aq) + HNO,(aq) → Cr³ * (aq)…

A: In simple words oxidation is reaction in which loss of electron takes place. Reduction is a reaction…

Q: Consider the following equation in aqueous solution: Cr:O,2 (aq) + S:O:² (aq) → Cr³*(aq) + S.O² (aq)…

A: The reaction is an oxidation reaction as electron is released by the reactant. Under acidic…

Concept explainers

Electrolysis

Electrolysis is defined as the process of breaking down ionic compounds into their constituent elements by passing a direct electric current through the compound in a fluid state. The cathode reduces cations, while the anode oxidizes anions. An electrolyte, electrodes, and some form of external power source are the main components required for conducting electrolysis. A partition, such as an ion-exchange membrane or a salt bridge, may also be used, but this is optional. These are primarily used to prevent the products from diffusing near the opposing electrode.

Question

4. For the following reactions:
Balance each equation using half-reactions in the given
conditions, and find the reduced and Oxidized reactants.
a. Al + NO3 → Al(OH)4 + NH3
(basic conditions)
b. Zn(s) + NO3(aq) → Zn+²(aq) + NH4 +(aq)
(acidic conditions)
C.
PbO2 (s) + 12(s) → Pb²+ (aq) +103- (aq)
(acidic conditions)
2-
d. MnO4 + Sn(OH)4²→→ Sn(OH)²- + MnO₂
(basic conditions)
e. CN- (aq) + CrO4)2(aq) →CNO- (aq) + Cr(OH)3 (s)
(basic conditions)

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

SEE SOLUTION Check out a sample Q&A here

Step 1: Oxidation and reduction

VIEW

Step 2: Rules to Balance redox reaction in acidic conditions

VIEW

Step 3: Balancing first reaction

VIEW

Step 4: Balancing first reaction

VIEW

Step 5: Balancing second reaction

VIEW

Step 6: Balancing third reaction

VIEW

Solution

VIEW

Step by step

Solved in 7 steps with 4 images

SEE SOLUTION Check out a sample Q&A here

Knowledge Booster

Learn more about

Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.

Similar questions

I. Balance the ff. redox reactions. Balance them using water in acidic medium if necessary. Cu+(aq) + Fe(s) → Fe3+(aq) + Cu(s)
3. In an electrochemical cell oxidation and reduction reactions occurs simultaneously, and it is these same reactions which generates electrical energy and powers the cell. a) Clearly identify the difference between an Oxidation and a Reduction reaction. b) Given the overall equation for the cell reaction: 2Cu*(aq) + I2 (aq) → 2Cu²*(aq) + 2I(aq) i. Identify the species which are the oxidizing agent and the reducing agent. Explain your answers. ii. Write the two half equations. iii. Draw the cell diagram iv. Calculate the standard cell e.m.f. v. Suggest whether the cell reaction is feasible. Explain your answer.
Hi, Balance each redox reaction using the half-reaction method, Al(s) + Ag+(aq) ------> Al3+(aq) + Ag(s) Thanks,
Write the oxidation and reduction half reactions for the following redox reaction. Make sure to label which is the oxidation and which is the reduction. (The number of electrons in both half reactions should be equal. You may balance the equation first if it helps you.) Al s)+HCI aq) → AIC 1, aq +H,(g) Write the ionic equation and net ionic equation for the following reaction. (Make sure to balance the equation.) Na,CO, aq+CaCl, aq) - NaCl aq+CaC O,(s) Determine the concentration in mol/L (M) of a solution of 19 25 g of LICLin acO O
Pls help with all the sub parts. Thanks!
Use the half-reaction to balance the following oxidation-reduction reaction. For the balanced equation, what is the sum of coefficients for the products? (your answer should be one number) As2O3 + CIO3 → H3ASO4 + Cl2 A/
Write two half‑reactions to describe each of these metal displacement reactions. Include phase symbols. Cancel out spectator ions. Cu(s)+2AuCl(aq)⟶CuCl2(aq)+2Au(s) oxidation half‑reaction: reduction half‑reaction:
Balance the following reaction in acidic solution. Cr2O, (ag) + HNO,(aq) → Cr* (aq) + NO, (aq) 3 Fill in the coefficients for the balanced overall equation. HNO, + -- v H* + -v Cr.O,* → -- ♥ NO, +- Cr3+ + Cr,O, - H.O --V
1,2,3
4. Determine whether each redox reaction occurs spontaneously in the forward direction. is SPOntancos a) Ni (s) + Zn2+ (aq) → Ni²+ (aq) + Zn (s) b) Ni (s) + Pb²+ (aq) → Ni²+ (aq) + Pb (s) c) Al (s) + 3 Ag* (aq) → 3 Al³+ (aq) + Ag (s) s2on tapeous d) Pb (s) + Mn2+ (aq) → Pb²+ (aq) + Mn (s)
Balance the following half-reactions by adding the appropriate number of electrons (e-). Then, classify each reaction as an oxidation or reduction half-reaction. Note that for each of the four reactions, one of the gray boxes will be left blank and the other will be filled with electron(s). Use the symbol e- to represent an electron. Part 4 + 12(s) + 6H2O(1) > 2I0-3 + 12H+(aq) + --
41. Balance each of the following equations according to the half-reaction method: (a) MnO4 (aq) + NO2 (aq) →→MnO2 (s) + NO3(aq) (in base) (b) MnO2 (aq)MnO4 (aq) + MnO2(s) (in base) (c) Br2(l) + SO2(g) → Br¯(aq) + SO4² (aq) (in acid)