Calculate the value of the equilibrium constant (Kc) for the reaction displayed if the following equilibrium concentration data were measured at 1200 K: [Br2(g)] = 0.0001151 mol/L, [Br(g)] = 0.00004423 mol/L.
Br2(g) = 2Br(g)
Kc = (Br)^2/(Br2)
Plug in the concns given and calculate.
To calculate the value of the equilibrium constant (Kc), we need to use the equilibrium concentrations of the reactants and products.
Given:
[Br2(g)] = 0.0001151 mol/L
[Br(g)] = 0.00004423 mol/L
The balanced chemical equation for the reaction is:
Br2(g) = 2Br(g)
In this equation, the stoichiometric coefficient of Br2(g) is 1, and the stoichiometric coefficient of Br(g) is 2.
Kc is calculated by taking the ratio of the product concentrations to the reactant concentrations, each raised to the power of their respective stoichiometric coefficients.
Kc = ([Br(g)]^2) / [Br2(g)]
Now, substitute the given equilibrium concentrations into the equation:
Kc = ([0.00004423 mol/L]^2) / [0.0001151 mol/L]
Kc = 0.000001959 mol^2/L^2 / 0.0001151 mol/L
Kc = 0.016987
Therefore, the value of the equilibrium constant (Kc) for the reaction is approximately 0.016987.