Question

Calculate the equilibrium constant Answer these questions please

1- N2(g) + 3H2(g) ⇌2NH3(g)

At equilibrium, the concentration of Nitrogen was 0.010M, the concentration of hydrogen was 0.025M and the concentration of ammonia was 0.15M. Calculate the equilibrium constant.


2- Calculate Kc given that, at equilibrium, the concentration of sulfur dioxide is

1.0 mol/L, the concentration of oxygen is 0.07 mol/L, and the concentration of sulfur trioxide is 0.06 mol/L.

2SO2(g) + O2(g) ⇌2SO3(g)


3-Calculate the equilibrium constant given the following concentrations at equilibrium: [Br2] = 0.05M, [Cl2] = 0.07M and [BrCl] = 0.06M

Br2(g) + Cl2(g) ⇌ 2BrCl(g)


4- When the Haber process is at equilibrium, there are 4 moles of nitrogen, 8 moles of hydrogen and 2 moles of ammonia in a 5L vessel. Calculate the equilibrium constant.

N2(g) + 3H2(g) ⇌2NH3(g)

Answer 1

1- The equilibrium constant for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) can be calculated using the concentration of the species at equilibrium:

Kc = [NH3]^2/([N2] * [H2]^3) = (0.15)^2/ (0.010 * (0.025)^3)

2- The equilibrium constant for the reaction 2SO2(g) + O2(g) ⇌ 2SO3(g) can be calculated using the concentration of the species at equilibrium:

Kc = [SO3]^2 / ([SO2] * [O2]) = (0.06)^2 / (1.0 * 0.07)

3- The equilibrium constant for the reaction Br2(g) + Cl2(g) ⇌ 2BrCl(g) can be calculated using the concentration of the species at equilibrium:

Kc = [BrCl]^2 / ([Br2] * [Cl2]) = (0.06)^2 / (0.05 * 0.07)

4- The equilibrium constant for the reaction N2(g) + 3H2(g) ⇌ 2NH3(g) can be calculated using the number of moles of the species at equilibrium and the volume of the vessel:

Kc = [NH3]^2/([N2] * [H2]^3) = (2/5)^2 / ((4/5) * (8/5)^3)