1. Calculate the value of Keg for this reaction at equilibrium.
2NOCl(g) <-> 2NO (g) +Cl2 (g)
An analysis of the equilibrium mixture in a 1-L flask gives the following results: NOCl, 0.30 mol; NO, 1.2 mol; 0.60 mol.
2. Carbon monoxide and hydrogen are combined in the commercial preparation of methyl alcohol.
CO (g) + 2H2 (g) <-> CH3OH 9g)
At a certain set of conditions, the equilibrium mixture contains 0.020 mol/L of CO, 0.60 mol/L of H2, and the equilibrium constant is 2.2 X 10^2. What is the concentrations of CH3OH in the equilibrium mixture?
2NOCl(g) <-> 2NO (g) +Cl2 (g)
An analysis of the equilibrium mixture in a 1-L flask gives the following results: NOCl, 0.30 mol; NO, 1.2 mol; 0.60 mol.
2. Carbon monoxide and hydrogen are combined in the commercial preparation of methyl alcohol.
CO (g) + 2H2 (g) <-> CH3OH 9g)
At a certain set of conditions, the equilibrium mixture contains 0.020 mol/L of CO, 0.60 mol/L of H2, and the equilibrium constant is 2.2 X 10^2. What is the concentrations of CH3OH in the equilibrium mixture?
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1. Keq = [NO]^2[Cl2]/[NOCl]^2
Keq = (1.2)^2(0.60)/(0.30)^2 = (1.44)(0.60)/(0.09) = 9.6
2. Keq = [CH3OH]/[CO][H2]^2
[CH3OH] = Keq[CO][H2]^2 = (2.2x10^2)(0.020)(0.36) = 1.6 mole to two significant figures
Keq = (1.2)^2(0.60)/(0.30)^2 = (1.44)(0.60)/(0.09) = 9.6
2. Keq = [CH3OH]/[CO][H2]^2
[CH3OH] = Keq[CO][H2]^2 = (2.2x10^2)(0.020)(0.36) = 1.6 mole to two significant figures