AnswersFoothill-B Period-Chemistry-2627BOxidizing and Reducing Agents

Oxidizing and Reducing Agents Answers

10 verified answers1 views
1
Free Preview

Which type of reaction occurs in the following equation? 2NO2(g) + 2OH(aq) NO(aq) + NO(aq) + H2O(l)

Question illustration
a
a combination redox reaction
a
a displacement redox reaction
a
a synthetic redox reaction
a
a disproportionation redox reaction
2
Free Preview

Zn(s) + 2H+(aq) Zn2+(aq) + H2(g) has an overall reduction potential of 0.76 V. Therefore,

Question illustration
t
the reaction is not spontaneous and will require energy to proceed.
t
the reaction is spontaneous and will proceed without any energy input.
t
the reduction potentials cancel out and prevent any reaction.
t
the forward and reverse reactions are each spontaneous.
3

Which type of reaction occurs in the following equation?3ClO(aq) ClO(aq) + 2Cl(aq)

Question illustration
a
an oxidation reaction
a
a reduction reaction
a
a synthesis reaction
a
a disproportionation reaction
4

Disproportionation is a process in which a substance

c
can act only as a reducing agent.
c
can act only as an oxidizing agent.
i
is both an oxidizing and a reducing agent.
i
is neither an oxidizing nor a reducing agent.
5

In the reaction equation BrO(aq) Br–(aq) + BrO(aq), how many oxidation states does the disproportionate substance have throughout the reaction?

Question illustration
0
0
1
1
2
2
3
3
6

Read the table below.Reduction Half-ReactionStandard Reduction Potential (V)Which reactants would lead to a spontaneous reaction?

Question illustration
M
Mn2+ and Cr
F
Fe and Cu2+
A
Al and Ba2+
M
Mg2+ and Sn
7

What describes the change in oxidation states of the following reaction?

Question illustration
C
Cl– reduces to Cl and F oxidizes to F–.
C
Cl– oxidizes to Cl and F reduces to F–.
C
Cl– is the reducing agent and F is the oxidizing agent.
C
Cl is the reducing agent and F– is the oxidizing agent.
8

During a redox reaction, the term reduction refers to

t
the gain of electrons.
t
the loss of electrons.
t
the gain of protons.
t
the loss of protons.
9

In a disproportionation reaction, the disproportionate substance

h
has exactly one oxidation state.
h
has exactly two oxidation states.
h
has at least three oxidation states.
h
has either one or two oxidation states.
10

Gold (Au) goes from an oxidation number of +3 to 0 in the reaction below.2Au3+ + 6I– 2Au + 3I2What describes the Au3+ ion?

Question illustration
I
It is the result of oxidation.
I
It the result of disproportionation.
I
It is the oxidizing agent.
I
It is the reducing agent.

Did you find these answers helpful?

More from this Course

Quiz
18 verified answers

Half-Life

Quiz
17 verified answers

Balancing Oxidation-Reduction Equations

Quiz
16 verified answers

Balancing Oxidation-Reduction Equations