Question

For each of the following reactions, calculate ΔH∘rxn, ΔS∘rxn, and ΔG∘rxn at 25 ∘C. State whether or not the reaction is spontaneous. If the reaction is not spontaneous, would a change in temperature make it spontaneous? If so, should the temperature be raised or lowered from 25 ∘C?

Part A

2CH4(g)→C2H6(g)+H2(g)

Express your answer to one decimal place.

ΔH∘rxn =

kJ

Part B

Calculate ΔS∘rxn at 25 ∘C.

Express your answer to one decimal place.

ΔS∘rxn =

J/K

Part D

2NH3(g)→N2H4(g)+H2(g)

Express your answer to one decimal place.

ΔH∘rxn =

kJ

Part E

Calculate ΔS∘rxn at 25 ∘C.

Express your answer to one decimal place.

ΔS∘rxn =

J/K

Part G

N2(g)+O2(g)→2NO(g)

Express your answer using three significant figures.

ΔH∘rxn =

kJ

Part H

Calculate ΔS∘rxn at 25 ∘C.

Express your answer to one decimal place.

ΔS∘rxn =

J/K

Part J

2KClO3(s)→2KCl(s)+3O2(g)

Express your answer to one decimal place.

ΔH∘rxn =

kJ

Part K

Calculate ΔS∘rxn at 25 ∘C.

Express your answer to one decimal place.

ΔS∘rxn =		J/K