Question

An equilibrium mixture of the reaction $2NO(g)+O_2(g)2N{O}_2(g)$ contains 0.12 moles of $N{O}_2$ , 0.08 moles of NO and 0.64 moles of 02 in a 4 litre flask at constant temperature. The value of $K_C$ this temperature is:

• A. 7
• B. 14
• C. 28
• D. 24

Answer 1

Answer: (B)

$\underset{Atequil0.08}{2NO(g)}+\underset{0.64}{O_2(g)}\underset{0.12}{2N{O}_2(g)},V=4litre$ $K_c=\frac{{[N{O}_2]}^2}{{[NO]}^2[O_2]}$ $=\frac{{\left(\frac{0.12}{4}\right)}^2}{{\left(\frac{0.08}{4}\right)}^2\times \left(\frac{0.64}{4}\right)}$ $=\frac{0.12\times 0.12\times 4}{0.08\times 0.08\times 0.64}=14.06$