Consider the following reaction, equilibrium concentrations, and equilibrium constant at a particular temperature. Determine the equilibrium concentration of H2O(g).
C2H4(g) + H2O(g) C2H5OH(g) Kc = 9.0 × 103
[C2H4]eq = 0.015 M [C2H5OH]eq = 1.69 M
So write the Keq expression, substitute the concentrations given and solve for the concn of H2O.
Post your work if you get stuck.
To determine the equilibrium concentration of H2O(g), we can use the equilibrium constant expression and the given equilibrium concentrations of C2H4 and C2H5OH.
The balanced chemical equation for the reaction is:
C2H4(g) + H2O(g) -> C2H5OH(g)
The equilibrium expression for the reaction is:
Kc = [C2H5OH]eq / ([C2H4]eq * [H2O]eq)
Given:
[C2H4]eq = 0.015 M
[C2H5OH]eq = 1.69 M
Kc = 9.0 × 103
Substituting the given equilibrium concentrations into the equilibrium expression:
9.0 × 103 = 1.69 / (0.015 * [H2O]eq)
Now, let's solve for [H2O]eq:
9.0 × 103 * 0.015 * [H2O]eq = 1.69
[H2O]eq = 1.69 / (9.0 × 103 * 0.015)
[H2O]eq ≈ 1.49 × 10^-5 M
Therefore, the equilibrium concentration of H2O(g) is approximately 1.49 × 10^-5 M.
To determine the equilibrium concentration of H2O(g), we can use the equilibrium constant, Kc, and the concentrations of the other species in the reaction.
The balanced chemical equation for the reaction is:
C2H4(g) + H2O(g) -> C2H5OH(g)
The equilibrium constant expression for this reaction is:
Kc = [C2H5OH]eq / ([C2H4]eq * [H2O]eq)
From the given information, we have:
[C2H4]eq = 0.015 M
[C2H5OH]eq = 1.69 M
Kc = 9.0 × 10^3
Now, we can rearrange the equilibrium constant expression to solve for [H2O]eq:
[H2O]eq = [C2H5OH]eq / (Kc * [C2H4]eq)
Plugging in the values:
[H2O]eq = 1.69 M / (9.0 × 10^3 * 0.015 M)
Calculating the value:
[H2O]eq ≈ 1.49 × 10^-5 M
Therefore, the equilibrium concentration of H2O(g) is approximately 1.49 × 10^-5 M.