The decomposition of nitrogen monoxide can be achieved under high temperatures to create the products of nitrogen and oxygen gas. 
6 NO(aq) ⇌ 3 N₂(aq) + 3 O₂(aq) 
a) What is the equilibrium equation for the reaction above?
b) What is the equilibrium expression for the reverse reaction. 

Ammonia reacts slowly in air to produce nitrogen monoxide and water vapor:

NH₃(g) + O₂(g) ⇌ NO(g) + H₂O(g) + Heat

b. Write the equilibrium equation.

State which is greater in amount: reactants or products, based on the given equilibrium constant, K.

a) N₂ (g) + O₂ (g) ⇌ 2 NO (g) K = 1.0 x 10²⁰

b) 2 CO (g) + O₂ (g) ⇌ 2 CO₂ (g) K = 2.2 x 10^-22

c) 2 BrCl (g) ⇌ Br₂ (g) + Cl₂ (g) K = 1

The equilibrium constant, K, for 2 NO (g) + O₂ (g) ⇌ 2 NO₂ (g) is 6.9 x 10². 

What is the [NO] in an equilibrium mixture of gaseous NO, O₂, and NO₂ at 500 K that contains 1.5 x 10 ^–2 M O₂ and 4.3 x 10 ^–3 M NO₂?

Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium.

c. Fe₂O₃(s) + 3 CO(g) ⇌ 2 Fe(s) + 3 CO₂(g) K (at 727 °C) = 24.2

Do the following reactions favor reactants or products at equilibrium? Give relative concentrations at equilibrium.

a. Sucrose(aq) + H₂O(l) ⇌ Glucose(aq) + Fructose(aq) K = 1.4 × 10⁵

The following diagrams represent two similar reactions that have achieved equilibrium:

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b. Calculate the value for the equilibrium constant for each reaction.