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= 7.0* 10^3
[C2H4]= 0.010M [C2H5OH]= 1.99M
Substitute (C2H4) and (C2H5OH) and Kc into the Kc expression and solve for (H2O)
what is the KC expression?
Kc = (C2H5OH)/(H2O)(C2H4)
To find the equilibrium concentration of H2O(g), you need to use the balanced chemical equation, the equilibrium constant (Kc), and the given equilibrium concentrations of the other reactants and products.
First, let's analyze the balanced chemical equation:
C2H4(g) + H2O(g) <--> C2H5OH(g)
According to the balanced equation, the stoichiometry of the reaction is 1:1:1 for C2H4, H2O, and C2H5OH.
Next, let's define the equilibrium concentrations:
[C2H4] = 0.010 M (concentration of C2H4 at equilibrium)
[C2H5OH] = 1.99 M (concentration of C2H5OH at equilibrium)
Now, let's use the equilibrium constant (Kc) to find the concentration of H2O(g). The equilibrium constant expression can be written as:
Kc = [C2H5OH] / ([C2H4] * [H2O])
Since the stoichiometry of the reaction is 1:1:1, the concentration of H2O can be represented as [H2O] itself.
Plugging in the given values into the equation, we have:
(7.0 * 10^3) = (1.99) / ((0.010) * [H2O])
Now, we can solve for [H2O]:
[H2O] = (1.99) / ((0.010) * (7.0 * 10^3))
[H2O] ≈ 0.028 M
Therefore, the equilibrium concentration of H2O(g) is approximately 0.028 M.