In the industrial synthesis of ammonia, the equilibrium constant expression may be written as: Keq= [NH3]^2/[N2][H2]^3
Calculate the value of this equilibrium constant, if the equilibrium concentration of nitrogen in the reaction mixture at 600°C if [N2] = 4.53 and [H2] = 2.49 M; [NH3] = 7.62 M
Keq = (NH3)^2/(N2)(H2)^3
Keq = (7.62)^2/(4.53)(2.49)^3 = about 0.830
n=0
To calculate the value of the equilibrium constant (Keq), we can substitute the given concentrations of reactants and products into the equilibrium constant expression:
Keq = [NH3]^2 / [N2][H2]^3
Plugging in the given values of [NH3] = 7.62 M, [N2] = 4.53 M, and [H2] = 2.49 M into the equation:
Keq = (7.62 M)^2 / (4.53 M)(2.49 M)^3
Simplifying:
Keq = 58.2044 M^2 / (4.53 M)(2.49 M)^3
Keq = 58.2044 M^2 / 4.53 M * (2.49 M)^3
Keq = 58.2044 M^2 / (4.53 M * 15.516881 M^3)
Keq = 58.2044 / (4.53 * 15.516881)
Keq = 58.2044 / 70.31253993
Keq ≈ 0.8278 (rounded to four decimal places)
Therefore, the value of the equilibrium constant (Keq) is approximately 0.8278.
To calculate the value of the equilibrium constant (Keq), you need to substitute the given equilibrium concentrations of nitrogen ([N2]), hydrogen ([H2]), and ammonia ([NH3]) into the equilibrium constant expression.
Given:
[N2] = 4.53 M
[H2] = 2.49 M
[NH3] = 7.62 M
The equilibrium constant expression is:
Keq = [NH3]^2 / ([N2] * [H2]^3)
Substituting the given values:
Keq = (7.62^2) / (4.53 * 2.49^3)
Calculating the denominator:
Keq = (58.1044) / (4.53 * 15.577431)
Keq = 58.1044 / 70.722401
Finally, calculating the value of Keq:
Keq ≈ 0.822 (rounded to three decimal places)
Therefore, the value of the equilibrium constant (Keq) is approximately 0.822.