Question

For the reaction, $N_{2\left(g\right)}+O_{2\left(g\right)}\leftrightharpoons 2N{O}_{\left(g\right)}$, the value of $K_c$ at ${800}^o$C is 0.1. When the equilibrium concentration of both the reactants is 0.5 mol, what is the value of $K_p$ at the same temperature?

• A. 0.5
• B. 0.1
• C. 0.01
• D. 0.025

Answer 1

The correct option is B 0.1

$K_P=K_c(RT{)}^{\Delta n}$
Here $\Delta n$ is the difference in the number of moles of gaseous products and the number of moles of gaseous reactants.
$K_P=0.1\times (RT{)}^{2-(1+1)}$
$K_P=0.1\times (RT{)}^0$
But $(RT{)}^0=1$

Hence, $K_p=0.1$