Question

Consider the following reaction:

Answer 1

Equation: NH4HS(s) <=> NH3 (g) + H2S(g)

Kc = [NH3]eq[H2S]eq; where eq subscripts are used to indicate that those are the concentrations at equilibrium

 Kc= 0.272 * 0.365 =0.09928

Answer 2

Answer : The equilibrium constant is, $9.928\times 10^{-2}$

Solution : Given,

Equilibrium concentration of $NH_3$ = 0.272 M

Equilibrium concentration of $H_2S$ = 0.365 M

The given balanced equilibrium reaction is,

$NH_4HS(s)\rightleftharpoons NH_3(g)+H_2S(g)$

The expression for equilibrium constant will be,

$K_c=\frac{[NH_3][H_2S]}{[NH_4HS]}$

Now put all the given values in this formula, we get  value of equilibrium constant.

$K_c=\frac{(0.272)\times (0.365)}{1}$

$K_c=0.09928=9.928\times 10^{-2}$

Therefore, the equilibrium constant is, $9.928\times 10^{-2}$