What are the equilibrium concentrations of each gas at 430 °C in a mixture of 0.437 M H2, 0.375 M I2, and 0.941 M HI, with a Kc value of 54.3?
To solve this Chemical Equilibrium problem, use the initial concentrations and the reaction stoichiometry to set up an equation based on the equilibrium constant expression. Solve the equation to find the change in concentrations (x), and substitute this back to find the equilibrium concentrations of H2, I2, and HI.
Calculation of Equilibrium Concentrations:
Initial concentrations:
[H2] = 0.437 M
[I2] = 0.375 M
[HI] = 0.941 M
Equilibrium concentrations:
[H2] = 0.437 - x
[I2] = 0.375 - x
[HI] = 0.941 + 2x
Using the equilibrium constant expression, Kc = [HI]^2 / ([H2] * [I2]), and substituting the equilibrium concentrations, we get 54.3 = (0.941 + 2x)^2 / ((0.437 - x) * (0.375 - x)). Solving this equation will give us the value of x, and we can then substitute x back into the equilibrium concentrations to find the final concentrations of each gas at the equilibrium.
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