AnswersEDG CHEM ES WLABS2P – Q2_9Oxidation-Reduction

Balancing Oxidation-Reduction Equations Answers

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1
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Which statement is true of the following reaction?

Question illustration
A
It is balanced for oxidation state and for number of atoms.
B
It is not balanced for oxidation state or for number of atoms.
C
It is not balanced for oxidation state but is balanced for number of atoms.
D
It is balanced for oxidation state but is not balanced for number of atoms.
2
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Which equation describes a reduction?

A
Upper M g (s) right arrow Uper M g superscript 2 plus (a q) plus 2 e superscript minus.
Option A
B
2 upper C l plus 2 e superscript minus right arrow 2 upper C l superscript minus.
Option B
C
Upper N a (s) right arrow upper N a superscript plus (a q) plus e superscript minus.
Option C
D
Upper A l (s) right arrow upper A l superscript 3 plus (a q) plus 3 e superscript minus.
Option D
3

What is the purpose of finding oxidation states in the half-reaction method for balancing equations?

A
to use as coefficients in the final equation
B
to identify the half reactions for the equation
C
to make sure the equation is balanced electrically
D
to find the electrons that are needed for each side of the equation
4

Consider the reaction below. Which half reaction correctly describes the reduction that is taking place?

Question illustration
A
Upper C l subscript 2 9 g) plus e superscript minus right arrow 2 upper C l superscript minu (a).
Option A
B
Upper C l subscript 2 (g) plus e superscript minus right arrow 2 upper C l superscript minus (a q).
Option B
C
2 upper I superscript minus (a q) right arrow upper I subscript 2 (a q) plus 2 e subscript minus.
Option C
D
2 upper I superscript minus (a q) right arrow upper I subscript 2 (a q) plus e superscript minus.
Option D
5

Consider the chemical reaction below. Zn(s) + 2H+(aq) Zn2+(aq) + H2(g)Which half reaction correctly represents reduction for this equation?

Question illustration
A
Zn(s) Zn2+(aq) + 2e–
Option A
B
2H+(aq) + 2e– H2(g)
Option B
C
Zn(s) Zn2+(aq) + e–
Option C
D
2H+(aq) + e– H2(g)
Option D
6

Consider the redox reaction below.Which half reaction correctly describes the oxidation that is taking place?

Question illustration
A
Upper Z n superscript 2 plus (s) plus 2 e superscript minus (a q) right arrow upper Z n (s).
Option A
B
Upper Z n (s) right arrow upper Z n superscript 2 plus (a q) plus 2 e superscript minus.
Option B
C
2 upper H superscript plus, plus 2 e superscript minus right arrow upper H subscript 2.
Option C
D
Upper H subscript 2 plus 2 e superscript minus right arrow 2 upper H superscript plus.
Option D
7

Equations can be balanced by using the half-reaction method. Which step should be completed immediately after finding the oxidation states of atoms?

A
inserting the coefficients
B
balancing the half reactions
C
identifying the half reactions
D
inspecting the number of atoms
8

The information below describes a redox reaction.What is the coefficient of silver in the final, balanced equation for this reaction?

Question illustration
A
1
B
2
C
3
D
4
9

Which half-reaction correctly describes an oxidation?

A
Upper C a (s) plus 2 e superscript minus right arrow upper C a superscript 2 plus (a q).
Option A
B
Upper B r subscript 2 plus 2 e superscript minus right arrow 2 upper B r superscript minus.
Option B
C
Upper N a superscript plus (a q) right arrow upper N a (s) plus e superscript minus.
Option C
D
Upper C r (s) right arrow upper C r superscript 3 plus (a q) plus 3 e superscript minus.
Option D
10

A student is asked to balance an equation by using the half-reaction method. He determines the two half reactions as shown below.What should he write as the final, balanced equation?

Question illustration
A
Upper C l subscript 2 plus 2 upper B r superscript minus right arrow upper B r subscript 2 plus 2 upper C l superscript minus.
Option A
B
Upper C l subscript 2 plus 2 upper B r superscript minus, plus 2 e superscript minus right arrow upper B r subscript 2 plus 2 upper C l superscript minus.
Option B
C
Upper C l subscript 2 plus 2 upper B r superscript minus right arrow upper B r subscript 2 plus 2 upper C l superscript minus, plus 2 e superscript minus.
Option C
D
Upper C l subscript 2 plus upper B r superscript minus plus 2 e superscript minus right arrow upper B r subscript 2 plus upper C l superscript minus, plus 2 e superscript minus.
Option D

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