Use the following data:
One mole each of A\(_2\)(g) and B\(_2\)(g) are taken in a \( 1 \) L closed flask and allowed to establish the equilibrium at \( 500 \) K.
\( \mathrm{A_2(g) + B_2(g) \rightleftharpoons 2\,AB(g)} \)
The value of \( x \) (in \( \mathrm{kJ\,mol^{-1}} \)) is __________. (Nearest Integer)
(Given: \( \log K = 2.2 \) \( R = 8.3 \\ \mathrm{J\,K^{-1}\,mol^{-1}} \))
