some nitrogen and hydrogen gases are pumped into an empty 5.00liter vessel at 500°c. when equilibrium was established, 3.00 moles of N2, 2.10 moles of H2 and 0.298 moles of NH3 were present. evaluate kc at 500°c
To find Kc at 500°C, we need to first write the balanced chemical equation for the reaction:
N2 + 3H2 ⇌ 2NH3
The equilibrium expression, with the concentration of each species raised to the power of its stoichiometric coefficient, is:
Kc = [NH3]^2 / ([N2]*[H2]^3)
We are given the moles of each species at equilibrium, but we need to convert them to their respective concentrations. Since the vessel is 5.00 liters, we can use the following conversions:
[N2] = 3.00 moles / 5.00 liters
[H2] = 2.10 moles / 5.00 liters
[NH3] = 0.298 moles / 5.00 liters
Now, substitute these values into the equilibrium expression:
Kc = (0.298/5.00)^2 / ((3.00/5.00)*(2.10/5.00)^3)
Evaluate this expression to find the value of Kc at 500°C.