For the following reaction at \( 50^{\circ}\text{C} \) and at \( 2 \, \text{atm} \) pressure,
\( 2\mathrm{N_2O_5(g)} \rightleftharpoons 2\mathrm{N_2O_4(g)} + \mathrm{O_2(g)} \)
\( \mathrm{N_2O_5} \) is \( 50\% \) dissociated.
The magnitude of standard free energy change at this temperature is \( x \). \( x = \_\_\_\_\_\_ \, \text{J mol}^{-1} \) [Nearest integer].
Given : \( R = 8.314 \, \text{J mol}^{-1}\text{K}^{-1} \), log \( 2 = 0.30 \), log \( 3 = 0.48 \), \( \ln 10 = 2.303 \), \( ^{\circ}\text{C} + 273 = \text{K} \)
