The expression for the reaction quotient , Q, is similar to that for equilibrim constant , Q, is similar to that for equilibrium constant K. The value of Q for the given composition of a reaction mixture helps us to know whether the reaction will move forward or backward or remain in equilibrium . It also helps to predict the effect of pressure on the direction of the gaseous reaction .In certain reactions, addition of inert gas also favours either the formation of reactants or products . The value of equilibrium constant of a reaction changes with change of temperature and the change is given by van't Hoff equation , d In `K_(p)//dT = Delta H^(@)//RT^(2)` where enthaply change, `DeltaH^(@)` , is taken as constant in the small temperature range.
The equilibrium constant for the reaction between `CH_(4)(g) and H_(2)S (g) " to form" CS_(2) (g) and H_(2) (g)`, at 1173 K is `3*6` . For the following composition of the reaction mixture , decide which of the following option is correct ?

Answer

C

Explanation

` CH_(4) (g) + 2 H_(2) S ( g) hArr CS_(2) (g) + 4 H_(2) (g) `
` Q_(c) = ((0*90) (1*78)^(2))/((1*97) (1*20))=5*86` ltbr gt As `Q_(c) gt K_(c)`, equilibrium will go in the backward direction.