Question

A certain process has ΔH° > 0, ΔS° < 0, and ΔG° > 0. The values of ΔH° and ΔS° do not depend on the temperature. Which of the following is a correct conclusion about this process? None of the above conclusions is correct. It is non-spontaneous at all T. It is spontaneous at low T. It is spontaneous at all T. It is spontaneous at high T

Answer 1

Answer: It is non-spontaneous at all T.

Step-by-step explanation:

According to Gibb's equation:

`\Delta G=\Delta H-T\Delta S`

`\Delta G` = Gibbs free energy = +ve

`\Delta H` = enthalpy change = +ve

`\Delta S` = entropy change = -ve

T = temperature in Kelvin

`\Delta G`= +ve, reaction is non spontaneous

`\Delta G`= -ve, reaction is spontaneous

`\Delta G`= 0, reaction is in equilibrium

Putting in the values:

`\Delta G=(+ve)-T(-ve)`

`\Delta G=(+ve)(+ve)=+ve`

Reaction is non spontaneous at all temperatures.