4HCl(g)+O2(g)-><-2Cl2(g)+2H2O(g) with Hcl=0.80M, Cl2=3.0M, O2=0.20M H2O=3.0M what is the equilibrium constant
What's your trouble with this. Substitute the concentrations into Kc expression and solve for K.
To find the equilibrium constant for this reaction, you need to use the law of mass action. The equilibrium constant, denoted as K, is defined as the ratio of the concentrations of the products to the concentrations of the reactants, with each concentration raised to the power of their respective stoichiometric coefficients.
For the given reaction 4HCl(g) + O2(g) <-> 2Cl2(g) + 2H2O(g), the equilibrium constant expression is:
K = [Cl2]^2 * [H2O]^2 / [HCl]^4 * [O2]
Now, substitute the given concentrations into the equilibrium constant expression:
K = (3.0M)^2 * (3.0M)^2 / (0.80M)^4 * (0.20M)
K = 9.0M * 9.0M / 0.4096M * 0.20M
K = 81M^2 / 0.08192M^2
K ≈ 978.52
Therefore, the equilibrium constant for this reaction is approximately 978.52.