The equilibrium system N2O4(g) 2NO2(g) was established in a 1.00-liter vessel. Upon analysis, the following information was found: [NO2] = 0.500 M; [N2O4] = 0.0250 M. What is the value of Keq?
To find the value of Keq (equilibrium constant) for the given equilibrium system, we need to use the concentrations of the reactants and products.
The equilibrium expression for the reaction N2O4(g) ⇌ 2NO2(g) is:
Keq = [NO2]^2 / [N2O4]
Given the concentrations of [NO2] = 0.500 M and [N2O4] = 0.0250 M, we can substitute these values into the equilibrium expression to calculate Keq.
Keq = (0.500 M)^2 / (0.0250 M)
Keq = 0.25 M / 0.0250 M
Keq = 10
So, the value of Keq for the given equilibrium system is 10.
N2O4 ==> 2NO2
Set up an ICE chart and substitute into the Keq expression. Solve for Keq. Post your work if you need additional help.