In a chemical reaction, 4 mol of nitrogen monoxide and 2.5 mol oxygen are mixed together in a container with a volume of 1000ml to produce nitrogen dioxide.lf the kc for this reaction is 0.001.
Determine the equilibrium concentrations for each substance?
The balanced chemical equation for the reaction is:
2NO(g) + O2(g) ⇌ 2NO2(g)
We are given the initial moles of NO and O2: 4 mol of NO and 2.5 mol of O2
We need to calculate the initial concentration for NO and O2:
Initial concentration of NO = 4 mol / (1000 ml / 1000) = 4 mol/L
Initial concentration of O2 = 2.5 mol / (1000 ml / 1000) = 2.5 mol/L
Since the initial concentration of products is 0, their concentrations are also 0.
To calculate the equilibrium concentrations, we'll use the equilibrium expression:
Kc = [NO2]^2 / ([NO]^2 * [O2])
We know that at equilibrium, the change in concentration for NO is -2x, O2 is -x and NO2 is +2x, where x is the change in concentration at equilibrium.
Substitute in the given values:
0.001 = (2x)^2 / ((4-2x)^2 * (2.5-x))
Solving this equation will give you the equilibrium concentrations for NO, O2, and NO2.