For the reaction taking place at a certain temperature $NH_2COONH_{4(s)} \rightleftharpoons 2NH_{3(g)} + CO_{2(g)}$,if the equilibrium pressure is $X \ bar$,then $\Delta_r G^o$ would be :-

At $300 \ K$,the equilibrium constant for a reaction is $10$. The standard free energy change (in $kJ \ mol^{-1}$) for the reaction is

Which of the following statements is correct for a reversible process in a state of equilibrium?

Of the following reactions:
$(i) \, A \rightleftharpoons B, \Delta G^{\circ} = 250 \, kJ \, mol^{-1}$
$(ii) \, D \rightleftharpoons E, \Delta G^{\circ} = -100 \, kJ \, mol^{-1}$
$(iii) \, F \rightleftharpoons G, \Delta G^{\circ} = -150 \, kJ \, mol^{-1}$
$(iv) \, M \rightleftharpoons N, \Delta G^{\circ} = 150 \, kJ \, mol^{-1}$
The reaction with the largest equilibrium constant is:

For a system in equilibrium,$\Delta G = 0$ under conditions of constant:

Hydrolysis of sucrose is given by the following reaction:
$\text{Sucrose} + H_{2}O \rightleftharpoons \text{Glucose} + \text{Fructose}$
If the equilibrium constant $(K_{c})$ is $2 \times 10^{13}$ at $300 \ K$,the value of $\Delta_{r}G^{\Theta}$ at the same temperature will be: