AnswersFoothill-B Period-Chemistry-2627BUnit Test

Unit Test Answers

15 verified answers
1
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Which substance loses electrons in a chemical reaction?

t
the one that is oxidized, which is the oxidizing agent
t
the one that is reduced, which is the reducing agent
t
the one that is oxidized, which is the reducing agent
t
the one that is reduced, which is the oxidizing agent
2
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What is the final, balanced equation that is formed by combining these two half reactions?

Question illustration
A
Option
Option A
B
Option
Option B
C
Option
Option C
D
Option
Option D
3

Equations can be balanced by using the half-reaction method. Which step should be completed first when using this method?

i
inserting the coefficients
b
balancing the half reactions
i
identifying the half reactions
f
finding the oxidation states of atoms
4

best

Question illustration
B
Bromine (Br) loses an electron, so it is the reducing agent.
B
Bromine (Br) gains an electron, so it is the reducing agent.
C
Chlorine (Cl) loses an electron, so it is the reducing agent.
C
Chlorine (Cl) gains an electron, so it is the reducing agent.
5

Look at the diagram of a fuel cell below.Which statement describes how electrons move if oxidation occurs on the left side of the cell and reduction occurs on the right side?

Question illustration
E
Electrons move from left to right through
E
Electrons move from right to left through A.
E
Electrons move from left to right through M.
E
Electrons move from right to left through M.
6

Consider the reaction that occurs when copper is added to nitric acid.Cu(s) + 4HNO3(aq) Cu(NO3)2(aq) + 2NO2(g) + 2H2O(l)What is the reducing agent in this reaction?

Question illustration
C
Cu
N
NO3–
C
Cu(NO3)2
N
NO2
7

Which of the following is a simple definition of reduction?

t
the loss of electrons
t
the gain of electrons
a
an agent that oxidizes something
a
an agent that reduces something
8

Hydrogen fuel cells that operate at lower temperatures use more expensive platinum electrode catalysts. What helps to make up for the higher-cost electrodes?

T
They use a cheaper fuel.
T
They operate at a higher efficiency.
T
They use a reaction that is not redox.
T
They produce fewer emissions.
9

Which of these is a direct benefit of using fuel cells in cars?

F
Fuel cells do not need an extra or rechargeable battery to operate the electronics.
F
Fuel cells use hydrogen gas, which can be safely stored in the car’s fuel tank.
F
Fuel cells use hydrogen gas, which is easily distributed throughout the country.
F
Fuel cells are inexpensive to construct and install in cars.
10

best

Question illustration
A
A silver ion gains electrons more easily and is a stronger oxidizing agent than a chromium(III) ion.
A
A silver ion loses electrons more easily and is a stronger oxidizing agent than a chromium(III) ion.
A
A silver ion gains electrons more easily and is a stronger reducing agent than a chromium(III) ion.
A
A silver ion loses electrons more easily and is a stronger reducing agent than a chromium(III) ion.
11

Look at the diagram of a fuel cell used to power a motorized vehicle.Which part of the fuel cell does A represent?

Question illustration
a
anode
c
cathode
e
electrolyte
m
motor
12

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Question illustration
I
Iron is being reduced.
I
Iron is being oxidized.
I
Iron is gaining electrons.
I
Iron is an oxidizing agent.
13

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

Question illustration
A
Option
Option A
B
Option
Option B
C
Option
Option C
D
Option
Option D
14

Given that Cu(s) + 2HCI(aq) Cu2+(aq) + 2CI–(aq) + H2(g) has an overall reduction potential of –0.34 V, what is a valid prediction about how this reaction works?

Question illustration
T
The reaction is not spontaneous and will require energy to proceed.
T
The reverse reaction would require energy input in order to occur.
T
The half reactions would both occur spontaneously.
T
The reaction is not spontaneous, and it is impossible to make it occur.
15

best

a
a reactant that undergoes oxidation
a
a reactant that undergoes reduction
t
the product of an oxidation
t
the product of a reduction

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