# 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 .

Express your answer using one decimal place and in kJ

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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 ...

#### Solution Summary

The expert examines entropy changes and equilibrium states.

Entropy Increase

How can ds = dqr/T (d-bar q(reversible) / T) can be used to determine the entropy increase of a system in an irreversible process. Why does this technique works?

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