Some N2 and H2 are placed in an empty 5.00 liter container at 500 degree celcius. When equilibrium is established, 3.0mol N2, 2.40mol H2 and 0.565mol of NH3 are present. Evaluate Kc for the reaction at 500 degree celcius.
N2 + 3H2 ==> 2NH3
At equilibrium,
(N2) = 3.0/5.00 = ?
(H2) = 2.40/5.00 = ?
(NH3) = 0.565/5.00 = ?
Substitute these equilibrium values into the Kc expression and evaluate Kc.
To evaluate Kc for the reaction, we first need to write the balanced equation:
N2 + 3H2 <=> 2NH3
The equation tells us that the stoichiometric coefficients for N2 and H2 are both 1, while the coefficient for NH3 is 2.
The equilibrium concentrations can be expressed as follows:
[N2] = 3.0 mol / 5.00 L = 0.60 mol/L
[H2] = 2.40 mol / 5.00 L = 0.48 mol/L
[NH3] = 0.565 mol / 5.00 L = 0.113 mol/L
Now we can calculate Kc using the concentrations:
Kc = ([NH3]^2) / ([N2] * [H2]^3)
Plugging in the values:
Kc = (0.113 mol/L)^2 / (0.60 mol/L * (0.48 mol/L)^3)
Calculating this:
Kc ≈ 0.020
Therefore, Kc for the reaction at 500 degrees Celsius is approximately 0.020.
To evaluate Kc for the reaction, we need to write down the balanced equation:
N2 + 3H2 ⇌ 2NH3
Now, we can determine the concentrations of N2, H2, and NH3 at equilibrium using the given information:
N2: 3.0 mol / 5.00 L = 0.60 M
H2: 2.40 mol / 5.00 L = 0.48 M
NH3: 0.565 mol / 5.00 L = 0.113 M
Next, we can use these equilibrium concentrations to calculate Kc.
Kc is determined by the concentrations of the products raised to their respective stoichiometric coefficients divided by the concentrations of the reactants raised to their respective stoichiometric coefficients.
Kc = [NH3]^2 / ([N2] * [H2]^3)
Substituting the values we obtained:
Kc = (0.113)^2 / (0.60 * 0.48^3)
= 0.0128 / 0.1106
≈ 0.1159
Therefore, the value of Kc for the reaction at 500 degrees Celsius is approximately 0.1159.