Question

Consider the inter conversion of nitrosotriaceto amine into nitrogen, phorone and water.


The reaction is $1^{st}$ order in each direction, with an equilibrium constant of ${10}^4$. The activation energy for the backward reaction is 57.45 kJ/mol. Assume its Arrhenius pre exponential factor as ${10}^{12}{s}^{-1}$.

Calculate $K_p$ of the reaction at 300 K

• A. $2.4\times {10}^{4}at{m}^{-1}$
• B. ${10}^{4}atm$
• C. $24.6\times {10}^{4}atm$
• D. $2.82\times {10}^{2}at{m}^{-1}$

Answer 1

The correct option is C $24.6\times {10}^{4}atm$

$K_p=K_c(RT{)}^{\Delta n}={10}^4(0.0821\times 300{)}^1=24.6\times {10}^4$