For the reaction A _ (g) → B _ (g) , the value of the equilibrium constant at 300K and 1atm is equal to 100 . 0 . The value of Δ G ^ o for the reaction at 300K and 1atm in Jmol ^ - 1 is - xR, where x is (Rounded off to

Correct answer: 0 Δ G ° = - RTlnKp = - R(300)(2) (10) = - R(300 × 2 × 2 .3) Δ G ° = - 1380R

JEE Main 202124 FebruaryMorning Shift

JEE Main 2021 · 24 February · Morning Shift · Chemistry · Thermodynamics (C)

For the reaction A _ (g) → B _ (g) , the value of the equilibrium...

For the reaction

{A}_{\left(g\right)} \to {B}_{\left(g\right)}

, the value of the equilibrium constant at

300K and 1atm

is equal to

100 . 0 .

The value of

{\Delta G}^{o}

for the reaction at

300K and 1atm in {Jmol}^{- 1}

- xR,

where

x

is (Rounded off to the nearest integer)

\left(R = 8 . 31J{mol}^{- 1}{K}^{- 1}andln10 = 2 . 3\right)

$\Delta G ° = - RTlnKp$

$= - R\left(300\right)\left(2\right)\ln \left(10\right)$

$= - R\left(300 \times 2 \times 2 .3\right)$

$\Delta G ° = - 1380R$