Use each equation to predict whether the relative entropy change is S (products) > S (reactants) or S (products) 0 or ΔS < 0 for the chemical reaction represented. Justify your answer in each case.

a. 2NH3 (g) →N2 (g) + 3H2 (g)

b. 2Al (s) + 3F2 (g) →2AlF3 (s)

Question

Jaylen Hernandez

Chemistry

18 October, 09:40

Use each equation to predict whether the relative entropy change is S (products) > S (reactants) or S (products) 0 or ΔS < 0 for the chemical reaction represented. Justify your answer in each case.

a. 2NH3 (g) →N2 (g) + 3H2 (g)

b. 2Al (s) + 3F2 (g) →2AlF3 (s)

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Answers (1)

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Monserrat Mathis · Answer 1

For reaction a, the mole number of gas increase from 2 to 4. So the entropy will increase, ΔS>0. For b, the gas will change to solid, so the entropy decrease, ΔS<0.

Use each equation to predict whether the relative entropy change is S (products) > S (reactants) or S (products) 0 or ΔS < 0 for the chemical reaction represented. Justify your answer in each case.a. 2NH3 (g) →N2 (g) + 3H2 (g)b. 2Al (s) + 3F2 (g) →2AlF3 (s)

Use each equation to predict whether the relative entropy change is S (products) > S (reactants) or S (products) 0 or ΔS < 0 for the chemical reaction represented. Justify your answer in each case.

a. 2NH3 (g) →N2 (g) + 3H2 (g)

b. 2Al (s) + 3F2 (g) →2AlF3 (s)