Question

A) Use the standard reduction potentials located in the 'Tables' linked above to calculate the standard free energy change in kJ for the reaction:

2Fe³⁺(aq) + Pb(s) ---> 2Fe²⁺(aq) + Pb²⁺(aq)

Answer: ____ kJ

K for this reaction would be ________ (greater/less) than one.

B) The free energy change for the following reaction at 25 °C, when [Hg²⁺] = 1.12 M and [H⁺] = 6.80×10^-3 M, is -178 kJ:

Hg²⁺(1.12 M) + H₂(g) ---> Hg(l) + 2H⁺(6.80×10^-3 M) ΔG = -178 kJ

What is the cell potential for the reaction as written under these conditions?

Answer: ____ V

Would this reaction be spontaneous in the forward or the reverse direction? ________ (forward/reverse)

C) Use the standard reduction potentials located in the 'Tables' linked above to calculate the equilibrium constant for the reaction:

Co²⁺(aq) + Hg(l) ----> Co(s) + Hg²⁺(aq)

Hint: Carry at least 5 significant figures during intermediate calculations to avoid round off error when taking the antilogarithm. You may use the OWL references to find the values you may need in this question.

Equilibrium constant: _____

DeltaG° for this reaction would be _________ (greater/less) than zero.

D) A standard galvanic cell is constructed in which a H⁺ | H₂ half cell acts as the cathode. Which of the following statements are correct?

Hint: Refer to a table of standard reduction potentials.

(Choose all that apply.)

- The anode reaction could be Mn -> Mn²⁺ + 2e^-

- In the external circuit, electrons flow from the other compartment to the H⁺|H₂ compartment.

- The anode compartment could be Cl₂|Cl^-.

- H⁺ is reduced at the cathode.

- The cathode reaction is H₂ -> 2H⁺ + 2e^-

Answer 1