Nitrogen and oxygen react at high temperatures.(a) Write the expression for the equilibrium constant (Kc) for the reversible reactionN2(g) + O2(g) ⇌ 2NO(g) ΔH = 181 kJ(b) What will happen to the concentrations of N2, O2, and NO at equilibrium if more O2 is added?(c) What will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed?(d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added?(e) What will happen to the concentrations of N2, O2, and NO at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?(f) What will happen to the concentrations of N2, O2, and NO at equilibrium if the temperature of the system is increased?(g) What will happen to the concentrations of N2, O2, and NO at equilibrium if a catalyst is added?
Nitrogen and oxygen react at high temperatures.
(a) Write the expression for the equilibrium constant (Kc) for the reversible reaction
N2(g) + O2(g) ⇌ 2NO(g) ΔH = 181 kJ
(b) What will happen to the concentrations of N2, O2, and NO at equilibrium if more O2 is added?
(c) What will happen to the concentrations of N2, O2, and NO at equilibrium if N2 is removed?
(d) What will happen to the concentrations of N2, O2, and NO at equilibrium if NO is added?
(e) What will happen to the concentrations of N2, O2, and NO at equilibrium if the pressure on the system is increased by reducing the volume of the reaction vessel?
(f) What will happen to the concentrations of N2, O2, and NO at equilibrium if the temperature of the system is increased?
(g) What will happen to the concentrations of N2, O2, and NO at equilibrium if a catalyst is added?
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