Any student is welcome to use this for extra practice and anyone is welcomed to amswed the question. Here is a couple of practice problems
a) 2 N2O(g) + O2(g) 4 NO(g)
B) H2(g) + CO2(g) H2O(g) + CO(g)
C) 4 HCl(g) + O2(g) 2 Cl2(g) + 2 H2O(g)
d) 3 H2(g) + N2(g) 2 NH3(g)
e) H2(g) + Cl2(g) 2HCl(g)
f) 2 SO2(g) + O2(g) 2 SO3(g)
If you are having a problem balancing these you need to tell us what the problem is. All appear to be balanced to me.
To determine the equilibrium constant expression for each of these reactions, we need to identify the concentrations or partial pressures of the reactants and products at equilibrium. The equilibrium constant expression is given by the concentrations of the products raised to their stoichiometric coefficients divided by the concentrations of the reactants raised to their stoichiometric coefficients.
For example, let's take reaction (a) 2 N2O(g) + O2(g) ↔ 4 NO(g)
The equilibrium constant expression for this reaction would be:
Kc = [NO]^4 / ([N2O]^2 * [O2])
Similarly, for the remaining reactions,
(b) H2(g) + CO2(g) ↔ H2O(g) + CO(g)
Kc = [H2O] * [CO] / ([H2] * [CO2])
(c) 4 HCl(g) + O2(g) ↔ 2 Cl2(g) + 2 H2O(g)
Kc = [Cl2]^2 * [H2O]^2 / ([HCl]^4 * [O2])
(d) 3 H2(g) + N2(g) ↔ 2 NH3(g)
Kc = [NH3]^2 / ([H2]^3 * [N2])
(e) H2(g) + Cl2(g) ↔ 2 HCl(g)
Kc = [HCl]^2 / ([H2] * [Cl2])
(f) 2 SO2(g) + O2(g) ↔ 2 SO3(g)
Kc = [SO3]^2 / ([SO2]^2 * [O2])
By plugging in the concentrations of the reactants and products at equilibrium and evaluating these expressions, you can calculate the equilibrium constant (Kc) for each reaction.