Question

For the reaction, $X_2{Y}_4\left(l\right)⟶2X{Y}_2\left(g\right)$ at 300 K, the values of $\Delta U$ and $\Delta S$ are 2 kcal and 20 cal $K^{-1}$ respectively. The value of $\Delta G$ for the reaction is

• A. - 3400 cal
• B. 3400 cal
• C. - 2800 cal
• D. 2000 cal

Answer 1

Answer: (C)

- 2800 cal

$\Delta H=\Delta U+\Delta n_{g}RT=2000+2\times 2\times 300=3200cal$

$\Delta G=\Delta H-T\Delta S=3200-300\times 20=-2800cal$