Deck 11: Electrochemistry

Question 1

An electrochemical system in which a 1.5 V battery supplies a current of 0.5 amps for 18 hours to an iron electrode immersed in a solution of nickel nitrate.

-Refer to Exhibit 17-2. What is the amount of electrical work done by the battery?

A) -72900 J
B) 72900 J
C) 122 J
D) -122 J
E) Not enough information provided
F) None of the above

Answer 1

72900 J

Question 2

An electrochemical system in which a 1.5 V battery supplies a current of 0.5 amps for 18 hours to an iron electrode immersed in a solution of nickel nitrate.


-Refer to Exhibit 17-2. How many moles of electrons flow through the wire?

A) 96485
B) 0.756
C) 0.504
D) 1.40´10^-4
E) None of the above

Answer 2

0.504

Question 3

An electrochemical system in which a 1.5 V battery supplies a current of 0.5 amps for 18 hours to an iron electrode immersed in a solution of nickel nitrate.


-Refer to Exhibit 17-2. If the iron electrode initially weighed 20.00 g, what is the mass after the flow of current is stopped?

A) 34.79 g
B) 34.07 g
C) 49.57 g
D) 5.22 g
E) 5.93 g

Answer 3

34.79 g

Question 4

The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M) Fe³⁺(0.200 M) + Ag(s)


-Refer to Exhibit 17-3. What is the value of "n" used in the Nernst equation for the reaction above?

A) 1
B) 2
C) 3
D) Not enough data given to answer the question
E) None of the above

Question 5

The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M) Fe³⁺(0.200 M) + Ag(s)


-Refer to Exhibit 17-3. What is the value of E°_cell for the reaction above?

A) .770
B) .296
C) .7996
D) None of the above

Question 6

The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M) Fe³⁺(0.200 M) + Ag(s)


-Refer to Exhibit 17-3. What is the value of the equilibrium constant, K, for the reaction above at 25°C?

A) 1.15
B) 3.17
C) .142
D) Not enough information is given to answer the question
E) None of the above

Question 7

The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M) Fe³⁺(0.200 M) + Ag(s)


-Refer to Exhibit 17-3. What is the value of the reaction quotient (Q) for this reaction?

A) 4.04
B) 1.11
C) 0.727
D) 0.248
E) Not enough information is given to answer the question
F) None of the above

Question 8

The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M) Fe³⁺(0.200 M) + Ag(s)


-Refer to Exhibit 17-3. Do you expect the silver electrode to gain mass or lose mass as the reaction approaches equilibrium?

A) Gain mass
B) Lose mass
C) Neither, solids do not appear in the equilibrium constant expression
D) Not enough information is given to answer the question
E) None of the above

Question 9

The electrochemical reaction below at 25°C.
Ag⁺(0.275 M) + Fe²⁺(0.180 M) Fe³⁺(0.200 M) + Ag(s)


-Refer to Exhibit 17-3. What will be the concentration of Fe³⁺ when the reaction reaches equilibrium?

A) 0.183 M
B) 0.217 M
C) 0.112 M
D) 0.290 M
E) None of the above

Question 10

The electrochemical reaction below at 25°C written in standard cell notation.
Pt|H₂ (1 atm)|H⁺(pH=1)||Cd²⁺(0.240 M)|Cd


-Refer to Exhibit 17-4. Which of the following is the chemical equation corresponding to the standard cell notation above?

A) Cd(s) + H₂(g) ? Cd²⁺(aq) + H⁺(aq)
B) Cd²⁺(aq) + H⁺(aq) ? Cd(s) + H₂(g)
C) Cd²⁺(aq) + H₂(g) ? H⁺(aq) + H⁺(aq)
D) H⁺(aq) + H⁺(aq) ? Cd²⁺(aq) + H₂(g)
E) None of the above

Question 11

The electrochemical reaction below at 25°C written in standard cell notation.
Pt|H₂ (1 atm)|H⁺(pH=1)||Cd²⁺(0.240 M)|Cd


-Refer to Exhibit 17-4. What is the value of E_cell ?

A) 0.414 V
B) 0.443 V
C) 0.662 V
D) 0.425 V
E) None of the above

Question 12

In the following equation

A)
0
B)

0
C) K = 1
D)

E) All of the above