Question

Mixing of $N_2$ and $H_2$ form an ideal gas mixture at room temperature in a container. For this process, which of the following statement is true?

• A. $\Delta H = 0,\ \Delta S_{surrounding}=0,\ \Delta S_{system}=0,\ \Delta G=-ve$
• B. $\Delta H = 0,\ \Delta S_{surrounding}=0,\ \Delta S_{system}>0,\ \Delta G=-ve$
• C. $\Delta H > 0,\ \Delta S_{surrounding}=0,\ \Delta S_{system}>0,\ \Delta G=-ve$
• D. $\Delta H < 0,\ \Delta S_{surrounding}>0,\ \Delta S_{system}<0,\ \Delta G=-ve$
• E. $\Delta H = 0,\ \Delta S_{surrounding}=0,\ \Delta S_{system}<0,\ \Delta G=-ve$

Hint:

Mixing of ideal gases always increases entropy.

Answer 1

The Correct Option is B