Question

When delta h is greater than 0 and delta s is less than 0. A reaction uis never spontaneous?

Answer 1

Answer: Yes, the given statement is true.

Explanation:

It is given that the $\Delta H$ is greater than zero, which means that the value of enthalpy change is positive.

And it is also given that $\Delta S$ is less than 0, which means that the value of entropy change is negative.

The expression for Gibb's Free energy is given by the equation:

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

where,

$\Delta G$ = Gibb's free energy change

$\Delta H$ = enthalpy change

T = temperature

$\Delta S$ = Entropy change

Putting the signs in above equation, we get:

$\Delta G=(+ve)-[T(-ve)]\\\\\Delta G=(+ve)(+ve)T\\\\\Delta G=+ve$

As, Gibb's free energy change is coming out to be positive, it means that the reaction is non-spontaneous.

Hence, the given statement is true.

Answer 2

Answer:

this is your answer

Explanation:

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