Balancing Oxidation-Reduction Equations

Question 1

Which element is oxidized? Which element is reduced? What is the oxidizing agent? What is the reducing agent?

Revolt · Accepted Answer

oxygen; Selection 1: oxygen; Selection 2: nitrogen; Selection 3: nitrogen; Selection 4: oxygen

Question 2

Which element is reduced?oxygen✔ nitrogenpotassium

Revolt · Accepted Answer

nitrogen

Question 3

What is the oxidizing agent?oxygen✔ nitrogenpotassium

Revolt · Accepted Answer

nitrogen

Question 4

What is the reducing agent?✔ oxygennitrogenpotassium

Revolt · Accepted Answer

oxygen

Question 5

Which pair of half-reactions represents the balanced half-reactions?

Revolt · Accepted Answer

First: upper n superscript 5 plus plus 4 e superscript minus right arrow 2 upper N superscript 3 plus. Second: 2 upper O superscript 2 minus right arrow upper O subscript 2 plus 4 e superscript minus.

Question 6

Consider this reaction and answer the questions: What is the oxidation number of chlorine in the reactant state? What is the oxidation number of oxygen in the reactant state? What is the oxidation number of potassium in the reactant state? What is the oxidation number of chlorine in the product state? What is the oxidation number of oxygen in the product state? What is the oxidation number of potassium in the product state?

Revolt · Accepted Answer

Part 1: +5; What is the oxidation number of oxygen in the reactant state?: -2; What is the oxidation number of potassium in the reactant state?: +1; What is the oxidation number of chlorine in the product state?: -1; What is the oxidation number of oxygen in the product state?: 0; What is the oxidation number of potassium in the product state?: +1

Question 7

Use the oxidation states as indicated by the superscript numbers to answer the questions. K(+1)Cl(+5)O3(-2) → K(+1)Cl(-1) + O2(0) Which element is oxidized? Which element is reduced? Which element does not change in the oxidation state? How many electrons will be moved to have a balanced reaction?

Revolt · Accepted Answer

Selection 1: oxygen; Selection 2: chlorine; Selection 3: potassium; Selection 4: 12

Question 8

Given the reaction Fe + O2 Fe2(3+)O3(2-), what happens to the oxidation states of these elements?Fe O

Revolt · Accepted Answer

Fe is oxidized from 0 to +3.; Selection 1: Fe is oxidized from 0 to +3.; Selection 2: O is reduced from 0 to –2.

Question 9

Based on the oxidation states of the atoms in this reaction, answer the questions. 4Fe(0) + 3O2(0) → 2Fe2(3+)O3(2-) How many electrons does the iron half-reaction lose? How many electrons does the oxygen half-reaction gain? What is the total number of electrons that are moved in this oxidation-reduction reaction?

Revolt · Accepted Answer

Part 1: 12; Part 2: 12; Part 3: 12

Question 10

Consider the reaction .Label the half-reactions as oxidation (use “O”) or reduction (use “R”).

Revolt · Accepted Answer

Consider the reaction .Label the half-reactions as oxidation (use “O”) or reduction (use “R”).: O; Part 2: R

Balancing Oxidation-Reduction Equations Answers

More from this Course

TRY EDGENUITY HACKS