Consider a reaction where S rxn = -315 J/K and H rxn = -45.6 kJ. Which statement

Question

Consider a reaction where S rxn = -315 J/K and H rxn = -45.6 kJ. Which statement is true about the spontaneity of this reaction?

a. This reaction is nonspontaneous at 25°C but will become spontaneous if the temperature is increased to 145°C.

b.This reaction is spontaneous at 25°C, but will become nonspontaneous if the temperature is decreased to -130°C.

c.This reaction is nonspontaneous at 25°C but will become spontaneous if the temperature is decreased to -130°C.

d.Decreasing the temperature will have no effect on the spontaneity of the reaction. It is nonspontaneous at 25°C and will become even less spontaneous as the temperature decreases.

Explanation / Answer

answer : This reaction is nonspontaneous at 25°C but will become spontaneous if the temperature is decreased to -130°C

S rxn = -315 J/K = - 0.315 kJ/K

H rxn = -45.6 kJ.

G = H - T x S

if the reaction is to be spontenous, G should be less than zero. or negative .

G < 0

0 < H - T x S

H < T x S

- 45.6 < T x - 0.315

145 K < T

- 128oC < T

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