Question

Consider a reaction that has a positive ΔH and a positive ΔS. Which of the following statements is TRUE?A) This reaction will be spontaneous only at high temperatures.B) This reaction will be spontaneous at all temperatures.C) This reaction will be nonspontaneous at all temperatures.D) This reaction will be nonspontaneous only at high temperatures.E) It is not possible to determine without more information.

Answer 1

Answer: A) This reaction will be spontaneous only at high temperatures

Explanation:

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

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

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

Using Gibbs Helmholtz equation:

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

Given : $\Delta H=+ve$

$\Delta S=+ve$

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

$\Delta G=(+ve)(-ve)$

Thus the value of  $\Delta G$  is negative and spontaneous when temperature is high.

Answer 2

The statements that is true is that  This reaction will be spontaneous only at high temperature.

What conditions does one have a reaction that is spontaneous?

Note that the condition that is necessary for one to have a spontaneous reaction is if ΔS > 0 and ΔH < 0.

Note also that the exothermic process is said to be spontaneous at any temperature. due to high temperature, there will be a reaction that is said to be spontaneous.

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