Chemical equilibrium constant expression (Kc).
2 NOCl (g) ↔2 NO (g) + Cl2 (g)
2 NOCl (g) ↔2 NO (g) + Cl2 (g)
These are easy to write. Here are the rules.
LHS = left hand side = reactants
RHS = right hand side = products
(x) = concentration of x (or whatever is inside)
Kc = (RHS^y/(LHS)^y
Kc = (NO)^2(Cl2)/(NOCl)^2
In words you do this. The product of the molar concentration of the products of the reaction divided by the product of the molar concentrations of the reactants, each raised to the power indicated by the coefficients in the balanced equation is a constant.
The equilibrium constant expression (Kc) for the given balanced chemical equation is:
Kc = [NO]^2 * [Cl2] / [NOCl]^2
In the equation, [NO] represents the molar concentration of NO gas, [Cl2] represents the molar concentration of Cl2 gas, and [NOCl] represents the molar concentration of NOCl gas. The coefficients in the balanced equation are used as exponents in the equilibrium constant expression.
To determine the equilibrium constant expression (Kc) for the given chemical equation, we need to understand the stoichiometry of the reaction.
The chemical equation is: 2 NOCl (g) ↔ 2 NO (g) + Cl2 (g)
The equilibrium constant expression (Kc) is defined as the ratio of the concentration of the products to the concentration of the reactants, with each concentration term raised to the power of its stoichiometric coefficient.
In this case, the stoichiometric coefficients of the reactants and products are:
Reactants:
NOCl(g) - coefficient of 2
Products:
NO(g) - coefficient of 2
Cl2(g) - coefficient of 1
Therefore, the equilibrium constant expression (Kc) for this reaction can be written as:
Kc = ([NO]^2 * [Cl2]) / [NOCl]^2
Where [NO], [Cl2], and [NOCl] represent the concentrations of NO, Cl2, and NOCl, respectively.
It is important to note that the concentrations should be written in terms of molarity (mol/L) and should be taken at the equilibrium state.
By plugging in the equilibrium concentrations of NO, Cl2, and NOCl into the equilibrium constant expression, you can calculate the value of Kc for a particular reaction under given conditions.