Question

For the reaction at ${25}^{o}C,X_2{O}_{4\left(l\right)}⟶2X{O}_{2\left(g\right)}$
$\Delta H=2.1kcal$ and $\Delta S=20cal{K}^{-1}$.

The reaction would be:

• A. spontaneous
• B. non-spontaneous
• C. at equilibrium
• D. unpredictable

Answer 1

The correct option is A spontaneous

Answer:- (A) Spontaneous

Given:-

T $={25}^{o}C=(273+25)K=298K$

$\Delta H=2.1kcal=2.1\times {10}^{3}cal\&\Delta S=20cal{K}^{-1}$

Gibbs free energy $\left(\Delta G\right)=\Delta H-T\Delta S$

$\Delta G=2.1\times {10}^3-(298\times 20)=2100-5960=-2860cal$

$\because \Delta G=negative$, thus the reaction is spontaneous.