You are given the following reaction and it's equilibrium constant at a given temperature.
2HBr + Cl2 2HCl+Br2
Kc=4.0*10^4
Write the expression for, and calculate the numerical value of, the equilibrium constant for each of the following at the same temperature.
4HBr +2Cl2 4HCl+2Br2
HBr+1/2Cl HCl+1/2Br2
To write the expression for the equilibrium constant for a given reaction, we need to write the equation for the reaction and include the concentrations of the reactants and products.
For the reaction: 2HBr + Cl2 ⇌ 2HCl + Br2
The expression for the equilibrium constant (Kc) is:
Kc = [HCl]^2[Br2] / [HBr]^2[Cl2]
Now, let's determine the expression for the equilibrium constant for each of the following reactions.
1) 4HBr + 2Cl2 ⇌ 4HCl + 2Br2
For this reaction, the expression for the equilibrium constant (Kc) is:
Kc = [HCl]^4[Br2]^2 / [HBr]^4[Cl2]^2
2) HBr + 1/2Cl2 ⇌ HCl + 1/2Br2
For this reaction, the expression for the equilibrium constant (Kc) is:
Kc = [HCl][Br2]/[HBr][Cl2]^0.5
To calculate the numerical value of the equilibrium constant for each reaction, we need to know the concentrations of the reactants and products. Without this information, we cannot calculate the specific numerical values.
To write the expression for the equilibrium constant for each of the given reactions, you need to make use of the stoichiometric coefficients in the balanced equation.
1. For the reaction: 4HBr + 2Cl2 → 4HCl + 2Br2
The expression for the equilibrium constant (Kc) is given by:
Kc = [HCl]^4 * [Br2]^2 / [HBr]^4 * [Cl2]^2
2. For the reaction: HBr + 1/2Cl2 → HCl + 1/2Br2
The expression for the equilibrium constant (Kc) is given by:
Kc = [HCl] * [Br2]^(1/2) / [HBr] * [Cl2]^(1/2)
Now, to calculate the numerical values of the equilibrium constants, you need more information about the concentrations of HBr, HCl, Cl2, and Br2 at the given temperature.