Question

Given the following reduction half-reactions:
Fe3+(aq)+e??Fe2+(aq)
E?red=+0.77V
S2O2?6(aq)+4H+(aq)+2e??2H2SO3(aq)
E?red=+0.60V
N2O(g)+2H+(aq)+2e??N2(g)+H2O(l)
E?red=?1.77V
VO+2(aq)+2H+(aq)+e??VO2+(aq)+H2O(l)
E?red=+1.00V

1.

Write balanced chemical equation for the oxidation ofFe2+(aq) byS2O2?6 (aq).

Express your answer as a chemical equation. Identify all of thephases in your answer.

2.

Calculate ?G? for this reaction at 298 K.

Express your answer using two significant figures.

3.

Calculate the equilibrium constant K for this reactionat 298 K.

Express your answer using one significant figure.

4.

Write balanced chemical equation for the oxidation ofFe2+(aq) byN2O(g).

Express your answer as a chemical equation. Identify all of thephases in your answer.

5.

Calculate ?G? for this reaction at 298 K.

Express your answer using three significant figures.

6.

Calculate the equilibrium constant K for this reactionat 298 K.

Express your answer using one significant figure.

7.Write balanced chemical equation for the oxidation ofFe2+(aq) byVO+2(aq).

8.

Calculate ?G? for this reaction at 298 K.

Express your answer using two significant figures.

9.

Calculate the equilibrium constant K for this reactionat 298 K.

Express your answer using one significant figure.