Question

For the reaction $N_{2(s)}+O_{2(s)} \rightleftharpoons 2 N O_{(g)}$, the value of $K_{c}$ at $800^{\circ} C$ is $0.1 .$ When the equilibrium concentrations 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

Answer: (B)

0.1

Answer 2

$N _{2}(g)+ O _{2}(g) \rightleftharpoons 2 NO (g)$
$K_{c}=0 . L_{p}=K_{c}(R T)^{\Delta n}$
$\Delta \,n=$ Number of gaseous product

- Number of gaseous reactants

$\Delta n=2-2=0 \quad \Delta n=0$
$\therefore K_{p}=K_{c}=0.1$