Question

For the equillibrium,
$2NOCl\left(g\right)\rightleftharpoons 2NO\left(g\right)+{Cl}_2\left(g\right)$
the value of equilibrium constant $K_c$ is $3.75{\times 10}^{-4}$ at $1069K$. Calculate the $K_p$ for the reaction at this temperature.

• A. $0.066$
• B. $3.33$
• C. $0.03$
• D. $0.033$

Answer 1

The correct option is B $3.33$

$K_P=K_C.(RT{)}^{\Delta ng}$

$\Rightarrow K_C=3.75\times {10}^{-4}$

$\Rightarrow T=1069K$

$\Delta ng$= moles of product- moles of reactant

$\Delta ng=3-2=1$

$\Rightarrow K_P=3.75\times {10}^{-4}\times (8.314\times 1069{)}^1$

$\Rightarrow K_P=3.33$