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9 Jun 2020

In the electrochemical reaction below, the value of is . What is the concentration of aluminum ions in a solution at equilibrium if the reaction begins with of solid aluminum and of zinc ions?

 

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General Chemistry 2
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Solve problems involving equilibrium calculations
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Related questions


1) Using the standard reduction potentials table in your book/notes, what is the standard change in gibbs free energy for the following reaction in kJ?

2NO3-(aq) + 8H+(aq) + 3Cu(s) → 3Cu2+(aq) + 2NO(g) + 4H2O(l)

If you took CHEM 122 lab here, this was the first reaction in the cycle of copper lab that released the brown NO gas.

2) What is the value of K at 298K for the following reaction? (Please give your answer to two significant digits in scientific notation) K = enFE°/RT

3A2+(aq) + 2B(s)→ 2B3+(aq) + 3A(s)

A2+(aq) + 2e- → A(s) E°red = −0.58 V

B3+(aq) + 3e- → B(s) E°red = − 0.75 V

3) What is the cell potential for the spontaneous concentration cell with the reaction Fe3+(aq) + Fe(s) → Fe(s) + Fe3+(aq), with concentrations of Fe3+ of 0.848M and 0.353M at a temperature of 310. K?

Ecell = E°cell −(RT/nF)lnQ

4) Which of the following will increase the cell potential for the following reaction:

2Fe3+(aq) + 3Zn(s) → 3Zn2+(aq) + 2Fe(s)

Use the reaction Ecell = E°cell − (RT/nF)lnQ and consider how each manipulation affects Q and thus affects Ecell

- Add zinc solid

- Remove water from the entire system

- Add solid iron to the system

- Increase the concentration of zinc ion in solution

- Dilute the entire system

- Increase the concentration of Fe3+ in the solution

A) What is the value of K at 298K for the following reaction? (Please give your answer to two significant digits in scientific notation) K = enFE°/RT

3A2+(aq) + 2B(s)→ 2B3+(aq) + 3A(s)

A2+(aq) + 2e- → A(s) E°red = −0.45 V

B3+(aq) + 3e- → B(s) E°red = − 0.75 V

B) Using the standard reduction potentials table in your book/notes, what is the standard change in gibbs free energy for the following reaction in kJ?

2NO3-(aq) + 8H+(aq) + 3Cu(s) → 3Cu2+(aq) + 2NO(g) + 4H2O(l)

If you took CHEM 122 lab here, this was the first reaction in the cycle of copper lab that released the brown NO gas.

C) What is the cell potential for the spontaneous concentration cell with the reaction Fe3+(aq) + Fe(s) → Fe(s) + Fe3+(aq), with concentrations of Fe3+ of 0.858M and 0.328M at a temperature of 310. K?

Ecell = E°cell −(RT/nF)lnQ

D)Which of the following will decrease the cell potential for the following reaction:

2Fe3+(aq) + 3Zn(s) → 3Zn2+(aq) + 2Fe(s)

Use the reaction Ecell = E°cell − (RT/nF)lnQ and consider how each manipulation affects Q and thus affects Ecell

Dilute the entire system

Remove water from the entire system

Add solid iron to the system

Increase concentration of Fe3+ in the solution

Increase the concentration of zinc ion in solution

Add zinc solid

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