Q: In an electrochemical cell, if aluminum is used as the anode, what is the overall charge transferred when $$2.8$$ moles of electrons are involved?

$$2.8 \times 96,485\ \mathrm{C}$$

Q: Which conversion factor is used to relate coulombs and joules in the context of electrical work?

$$1\ \mathrm{J} = 1\ \mathrm{C} \times 1\ \mathrm{V}$$

Question 1

Which equation correctly relates the standard cell potential ($$E_{cell}$$), the number of moles of electrons transferred ($$n$$), and the Gibbs Free Energy change ($$\Delta G) $$for an electrochemical cell?

Accepted Answer

$$\Delta G = -nFE_{cell}$$

Question 2

A galvanic cell is constructed using the following half-reactions:

$$\mathrm{Au$$^{3+}$$ + 3e^- \rightarrow Au}$$ ($$E^\circ = 1.50\ \mathrm{V}$$)

$$\mathrm{Al$$^{3+}$$ + 3e^- \rightarrow Al}$$ ($$E^\circ = -1.66\ \mathrm{V})

$$Which metal acts as the anode?

Accepted Answer

Aluminum (Al)

Question 3

If the standard cell potential for a reaction is $$+2.24\ \mathrm{V}$$ and $$6$$ moles of electrons are transferred, what is the maximum electrical work (in kJ) that can be produced by the cell? ($$F = 96,485\ \mathrm{C/mol})$$

Accepted Answer

$$-1,295\ \mathrm{kJ}$$

Question 4

Faraday's constant ($$F) is $$defined as the charge carried by one mole of electrons. What is its value in coulombs per mole?

Accepted Answer

$$96,485\ \mathrm{C/mol}$$

Question 5

In an electrochemical cell, if aluminum is used as the anode, what is the overall charge transferred when $$2.8$$ moles of electrons are involved?

Accepted Answer

$$2.8 	imes 96,485\ \mathrm{C}$$

Question 6

Given the reaction $$\mathrm{Au$$^{3+}$$ + 3e^- \rightarrow Au}$$ and $$\mathrm{Al \rightarrow Al$$^{3+}$$ + 3e^-}$$, what is the standard cell potential ($$E^\circ_{cell}) if$$ $$E^\circ_{Au$$^{3+}$$/Au} = 1.50\ \mathrm{V}$$ and $$E^\circ_{Al$$^{3+}$$/Al} = -1.66\ \mathrm{V}$$?

Accepted Answer

$$2.24\ \mathrm{V}$$

Question 7

A cell is constructed with the following half-reactions:

$$\mathrm{$$ClO_3$$^- + 6H^+ + 6e^- \rightarrow Cl^- + 3H_2O}

If $$the standard cell potential is $$1.37\ \mathrm{V}$$, how many electrons are transferred in the reaction?

Accepted Answer

6

Question 8

Which of the following best describes the role of the cathode in a galvanic cell?

Accepted Answer

It is where reduction occurs.

Question 9

If $$1.5$$ moles of electrons are transferred in an electrochemical reaction, what is the total charge in coulombs?

Accepted Answer

$$144,728\ \mathrm{C}$$

Question 10

Which of the following statements about Gibbs Free Energy ($$\Delta G) $$and cell potential ($$E_{cell}) is $$correct?

Accepted Answer

A positive $$E_{cell}$$ corresponds to a negative $$\Delta G$$, indicating a spontaneous reaction.

Question 11

If the cell reaction is $$\mathrm{Au$$^{3+}$$ + Al \rightarrow Au + Al$$^{3+}$$}$$ and $$E^\circ_{cell} = 2.24\ \mathrm{V}$$, how much energy (in kJ) is released when $$2$$ moles of electrons are transferred?

Accepted Answer

$$-432\ \mathrm{kJ}$$

Question 12

Which conversion factor is used to relate coulombs and joules in the context of electrical work?

Accepted Answer

$$1\ \mathrm{J} = 1\ \mathrm{C} 	imes 1\ \mathrm{V}$$

Question 13

In a cell where $$E^\circ_{cell} is $$negative, what can be said about the spontaneity of the reaction?

Accepted Answer

The reaction is non-spontaneous.

Question 14

If $$E^\circ_{cell} = 1.37\ \mathrm{V}$$ and $$n = 6$$, what is the value of $$\Delta G in kJ$$? ($$F = 96,485\ \mathrm{C/mol})$$

Accepted Answer

$$-794\ \mathrm{kJ}$$

Question 15

Which of the following is the correct definition of Faraday's constant?

Accepted Answer

The charge of one mole of electrons.

Question 16

A cell reaction involves $$3$$ moles of electrons and has a cell potential of $$0.50\ \mathrm{V}. $$What is the Gibbs Free Energy change ($$\Delta G) in kJ$$? ($$F = 96,485\ \mathrm{C/mol})$$

Accepted Answer

$$-144.7\ \mathrm{kJ}$$

Question 17

Which of the following best describes the relationship between cell potential and the direction of electron flow in a galvanic cell?

Accepted Answer

Electrons flow from the anode to the cathode.

Electrochemistry: Cell Potential, Gibbs Free Energy, and Faraday’s Constant

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