Read the passage given below and answer the questions from 36-37:
\( \mathrm{P} \)
The concentration ratio i.e., ratio of the product of concentrations of products to that of reactants is also known as concentration quotient and is denoted by Concentration quotient, \( \mathrm{Q}=([\mathrm{C}][\mathrm{D}]) /([\mathrm{A}][\mathrm{B}]) \).It may be noted that \( \mathrm{Q} \) becomes equal to equilibrium constant \( (\mathrm{K}) \) when the reaction is at the equilibrium state. Thus, at equilibrium, \( Q \) \( =\mathrm{K} \)
For the chemical reaction, \( \mathrm{H}_{2}+\mathrm{I}_{2} \rightleftharpoons 2 \mathrm{HI} \) \( \mathrm{K}_{\mathrm{p}} \) for the reaction is 0.25 . If 0.4 moles each of \( \mathrm{H}_{2} \) and \( \mathrm{I}_{2} \) are present, and 2 moles of \( \mathrm{HI} \) are present, then in which direction the reaction proceeds?
(1) Forward
(2) Backward
(3) Already at equilibrium
(4) None of these
0