7. Energy, Rate and Equilibrium

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 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. 

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.

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

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a. Write the expression for the equilibrium constant for each reaction.