The numerical value of equilibrium constant is very important because it helps us to know whether we expect a reaction mixture at equilibrium to contain a high or a low concentration of products. Equilibrium constant helps us to predict the extent of reaction, direction of reaction and to calculate equilibrium concentrations.
The equilibrium constant for the reaction `N_(2(g)) + 3H_(2(g))

Options

A. `0.25 mol L^(-1)`
B. `0.11 mol L^(-1)`
C. `2.5 mol L^(-1)`
D. ` 3.84 mol L^(-1)`

Answer

D

Explanation

`K_c = ([NH_3]^2)/([N_2][H_2]^3)`
`implies 6.0 xx 10^(-2) = ((0.06)^2)/([N_2][0.25]^3)`
`implies [N_2] = (0.06 xx 0.06)/(6 xx 10^(-2) xx 0.25 xx 0.25 xx 0.25)`
`implies [N_2] = 3.84 mol L^(-1)`