For the reaction $\mathrm{A}_{(g)} \rightarrow \mathrm{B}_{(\mathrm{g})}$, the value of the equilibrium constant at $300 \mathrm{~K}$ and $1 \mathrm{~atm}$ is equal to $100.0$. The value of $\Delta_{r} G$ for the reaction at $300 \mathrm{~K}$ and 1 atm in $\mathrm{Jmol}^{-1}$ is $-\mathrm{xR}$, where $\mathrm{x}$ is__________________. (Rounded off to the nearest integer)
$\left[\mathrm{R}=8.31 \mathrm{~J} \mathrm{~mol}^{-1} \mathrm{~K}^{-1}\right.$ and $\left.\ln 10=2.3\right]$
(1380)
$\Delta G^{\circ}=-R T$ In Keq.
$=-R \times 300 \times \ln \left(10^{2}\right)$
$=300 \times 2 \times 2.3 \times(-R)$
$=-1380 \mathrm{R}$
$x=1380$ ans.
Click here to get exam-ready with eSaral
For making your preparation journey smoother of JEE, NEET and Class 8 to 10, grab our app now.