5.0 mol of nitrogen gas is reacted with 2.5 mol of oxygen gas in an 10. L container. At equilibrium, 1.5 mol of nitrogen dioxide is collected.What is the equilibrium constant for the formation of NO2 gas?
The equilibrium constant for the NO2 reaction formation is 0.52
Explanation:
First is needed the balanced reaction equation: N2 + 2 O2 = 2 NO2.
With the information provided from the equation, is possible to know that to produce the 1.5 mol of NO2, were required 0.75 mol of N2 and 1.5 mol of O2.
That means that in equilibrium there would be in the container: (5 - 0.75 = 4.25) mol of N2, (2.5 - 1.5 = 1) mol of O2 and 1.5 mol of NO2.
By definition the equilibrium constant for this reaction would be: [tex]k_c=\frac{[NO_2]^2}{[N_2][O_2]^2}[/tex], where each term represents the equilibrium moles of each species, and the exponents are the respective stoichiometric coefficient for each species in the reaction equation.
Then replacing in the expression the calculated moles of each component in equilibrium: ,[tex]k_c=\frac{[NO_2]^2}{[N_2][O_2]^2}=\frac{[1.5]^2}{[4.25][1]^2}=0.52[/tex]
