Question

$2NO\left(g\right)+C{l}_2\left(g\right)\rightleftharpoons 2NOCl\left(g\right)K=4.6\times {10}^4$
$\left[NO\right]=1.00M;\left[C{l}_2\right]=1.00M;\left[NOCl\right]=0M$

• A. 0, shifts right
• B. 10, shifts right
• C. 1, shifts right
• D. $Noneofthese$

Answer 1

Answer: (A)

0, shifts right

The reaction quotient $Q=\frac{[NOCl{]}^2}{\left[NO{]}^2\right[C{l}_2]}=\frac{0^2}{1^2\times 1}=0$

But the equilibrium constant $K=4.6\times {10}^4$

Hence, the reaction quotient Q is smaller than the equilibrium constant K

$Q<K$

Hence, the concentration of products is smaller than the equilibrium concentration and the concentration of reactants is higher than the equilibrium concentration.

The system will shift right to reach equilibrium till Q becomes equal to K.