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# Entropy Changes and Equilibrium states

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CHM4
1- Calculate the standard entropy change for the reaction
2Na(s)+Cl 2 (g)→2NaCl(s)
using the data from the following table:
Substance ΔH ∘ f (kJ/mol)
ΔG ∘ f (kJ/mol)
S ∘ [J/(K⋅mol)]

Na(s)
0.00 0.00 51.30
Cl 2 (g)
0.00 0.00 223.1
NaCl(s)
-411.0 -384.0 72.10
Express your answer to four significant figures and include the appropriate units.

2 - Use data from Appendix IIB in the textbook to calculate the equilibrium constants at 25 ∘ C for each reaction.2H 2 S(g)⇌2H 2 (g)+S 2 (g) Express your answer using two significant figures.I have provided the data below.

delta G for N2 - 0
delta H for N2 - 0
delta S for N2 - 191.6

delta G for O2 - 0
delta H for O2 - 0
S for O2 - 205.2

delta G for 2NO - 87.6
delta H for 2NO - 91.3
S for 2NO - 210.8

Consider the reaction:
I 2 (g)+Cl 2 (g)⇌2ICl(g)
K p = 81.9 at 25 ∘ C .
Calculate ΔG rxn for the reaction at 25 ∘ C under each condition:
Part A: standard conditions Express your answer using one decimal place and in kJ
Part B: at equilibrium
Part C:
P ICl = 2.55atm ;
P I 2 = 0.315atm ;
P Cl 2 = 0.219atm .

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CHM4
1- Calculate the standard entropy change for the reaction
2Na(s)+Cl 2 (g)→2NaCl(s)
using the data from the following table:
Substance ΔH ∘ f (kJ/mol)
ΔG ∘ f (kJ/mol)
S ∘ [J/(K⋅mol)]

Na(s)
0.00 0.00 51.30
Cl 2 (g)
0.00 0.00 223.1
NaCl(s)
-411.0 -384.0 72.10
Express your answer to four significant figures and include the appropriate units.
ΔSo = [2 x ...

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