If δh = - 70.0 kj and δs = - 0.500 kj/k, the reaction is spontaneous below a certain temperature. calculate that temperature. express your answer numerically in kelvins.

Question

Braxton Coleman

Chemistry

30 April, 07:48

If δh = - 70.0 kj and δs = - 0.500 kj/k, the reaction is spontaneous below a certain temperature. calculate that temperature. express your answer numerically in kelvins.

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Answers (1)

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Jordan Jacobs · Answer 1

Answer is: temperature must be less than 140 K.

Gibbs free energy (G) determines if reaction will proceed spontaneously. If the value of G is a negative, the reaction is spontaneous. ΔG = ΔH - T·ΔS.

ΔH = - 70.00 kJ.

ΔS = - 0.500 kJ/K.

-70 kJ = T · (-0.5 kJ/K).

T = - 70.00 kJ : (-0.500 kJ/K).

T = 140 K.