\( 37.8 \ \mathrm{g} \ \mathrm{N_2O_5} \) was taken in a \( 1 \ \mathrm{L} \) reaction vessel and allowed to undergo the following reaction at \( 500 \ \mathrm{K} \)
\( 2 \ \mathrm{N_2O_5(g)} \rightleftharpoons 2 \ \mathrm{N_2O_4(g)} + \mathrm{O_2(g)} \)
The total pressure at equilibrium was found to be \( 18.65 \ \mathrm{bar} \).
Then, \( K_p = \_\_\_\_\_\_\_\_\_\_ \times 10^{-2} \) [nearest integer] Assume \( \mathrm{N_2O_5} \) to behave ideally under these conditions.
Given: \( R = 0.082 \ \mathrm{bar \ L \ mol^{-1} \ K^{-1}} \)
