One mole each of He and A ( g ) are taken in a 10 L closed flask and heated to 400 K to establish the following equilibrium. A ( g ) ⇌ B ( g ) K_c…

One mole each of He and $\displaystyle \mathrm{A}(\mathrm{g})$ are taken in a $\displaystyle 10$ L closed flask and heated to $\displaystyle 400$ K to establish the following equilibrium. $\displaystyle \mathrm{A}(\mathrm{g}) \rightleftharpoons \mathrm{B}(\mathrm{g})$ $\displaystyle \mathrm{K}_{\mathrm{c}}$ for this reaction at $\displaystyle 400$ K is 4.0. The partial pressures (in atm) of He and B(g) are respectively (at equilibrium) (Assume $\displaystyle \mathrm{He}, \mathrm{A}(\mathrm{g})$ and $\displaystyle \mathrm{B}(\mathrm{g})$ behave as ideal gases) (Given : $\displaystyle \mathrm{R}=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}$ )