Answer to Question #129433 in Physical Chemistry for Jason

Question

Consider the following reversible reaction occurring in a 1.00 L
enclosed vessel:
(NH4)2SO4(s) to 2NH3(g) + H2SO4(g)
Given that the value of the equilibrium constant, Kc, of this reaction is
2.57 × 10-5
, calculate the molar concentrations of NH3(g) and H2SO4(g)
at equilibrium. No NH3(g) and H2SO4(g) were present initially.

Answer 1

Let concentration of H₂SO₄ IS X.

CONCENTRATION OF NH₃ IS 2X.

So , Equillibrium Constant ( K_c ) . = (2X)² . (X)¹ . = 4(X)³ .

4X³ = 2.57 * 10^-5 ..

X = 2.57 * 10^-5 / 4 .

X = 6 * 10^-6 .

Concentration of H₂SO₄ . = X = 6 * 10^-6 .

Concentration of NH₃ = 2X = 12 * 10^-6 .