1. Tardigrade
  2. Question
  3. Chemistry
  4. At 700 K, the equilibrium constant, K p , for the reaction 2 SO 3( g ) rightharpoons 2 SO 2( g )+ O 2( g ) is 1.8 × 10-3 atm. The value of K c for the above reaction at the same temperature in moles per litre would be

Question Error Report

Thank you for reporting, we will resolve it shortly

Back to Question

Q. At $700 \,K$, the equilibrium constant, $K _{ p }$, for the reaction $2 SO _{3}( g ) \leftrightharpoons 2 SO _{2}( g )+ O _{2}( g )$ is $1.8 \times 10^{-3} atm$. The value of $K _{ c }$ for the above reaction at the same temperature in moles per litre would be

Equilibrium

Solution:

For the reaction,
$\Delta n=1 $
$\therefore K_{p}=K_{c}(R T)^{\Delta n}=K_{c} R T $
$\therefore K_{c}=\frac{K_{p}}{R T}$
$=\frac{1.8 \times 10^{-3} atm }{0.082\, L \,a t m \,K ^{-1} mol ^{-1} \times 700\, K }=3.13 \times 10^{-5}$