Problem 20.51

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

Part A

Write balanced chemical equation for the oxidation ofFe2+(aq) by S2O2?6 (aq).

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

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Part B

Calculate ?G? for this reaction at 298 K.

Express your answer using two significant figures.

?G? =		  kJ Â

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Part C

Calculate the equilibrium constant K for this reactionat 298 K.

Express your answer using one significant figure.

K =

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Part D

Write balanced chemical equation for the oxidation ofFe2+(aq) by N2O(g).

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

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Part E

Calculate ?G? for this reaction at 298 K.

Express your answer using three significant figures.

?G? =		  kJ Â

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Part F

Calculate the equilibrium constant K for this reactionat 298 K.

Express your answer using one significant figure.

K =

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Part G

Write balanced chemical equation for the oxidation ofFe2+(aq) by VO+2(aq).

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

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Part H

Calculate ?G? for this reaction at 298 K.

Express your answer using two significant figures.

?G? =		  kJ Â

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Part I

Calculate the equilibrium constant K for this reactionat 298 K.

Express your answer using one significant figure.

K =