The equilibrium 2no(g)+cl2(g)⇌2nocl(g) is established at 500 k. an equilibrium mixture of the three gases has partial pressures of 9.30×10−2 atm , 0.174 atm , and 0.25 atm for no, cl2, and nocl, respectively. calculate kp for this reaction at 500 k. then if the vessel has a volume of 5.20 l calculate kc.

Kp = 41.53

Kc = 1.01

Explanation:

To calculate the equilibrium constant in terms of pressure, what we simply do is to use the equilibrium pressure raised to the power of the number of moles. What we are saying in essence is this:

Kp = [NOCl]^2/[NO]^2[Cl]

Kp= [0.25]^2/[0.174][0.093]^2 = 41.53

Kp = Kc (RT)^Dn

Hence, Kc = Kp/[RT]^(delta n )^-1

n = sum of the number of moles of products minus the sum of the number of moles of reactants= 2-3 = -1 in this case

Kc = 41.53/(0.0821 * 500)^1

Kc = 1.01

true

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