In a chemical reaction ,4 Mol of nitrogen monooxide (No) and 2.5 mol of oxygen (O2) are mixed together in a container with a volume of 1000ml to produce Nitrogen Dioxide (NO2).If the Kc ( equilibrium constant) foe this reaction is 0.001.
Determine the equilibrium constant for each substance?
The balanced chemical equation for the reaction is:
2NO (g) + O2 (g) -> 2NO2 (g)
At equilibrium, the reaction quotient Qc is calculated as follows:
Qc = [NO2]^2 / ([NO]^2 [O2])
Given that the initial moles of NO is 4 mol, initial moles of O2 is 2.5 mol, and the volume of the container is 1000 ml, we can calculate the initial concentrations of each substance:
[NO] = 4 mol / 1 L = 4 M
[O2] = 2.5 mol / 1 L = 2.5 M
Next, we can calculate the equilibrium concentrations of each substance using the stoichiometry of the balanced equation:
2NO (g) + O2 (g) -> 2NO2 (g)
Since the stoichiometry of the reaction is 1:1:2, the equilibrium concentrations are:
[NO] = 4 - 2x mol/L
[O2] = 2.5 - x mol/L
[NO2] = 2x mol/L
Substitute these values into the reaction quotient equation Qc:
Qc = (2x)^2 / ((4 - 2x)^2 (2.5 - x))
Given that Kc = 0.001 at equilibrium, we can set Qc = 0.001 and solve for x to find the equilibrium concentrations of each substance.
After solving for x, we will get the equilibrium concentrations of [NO], [O2], and [NO2].