Equilibrium Constants

When 0.40 mole of SO₂ and 0.60 mole of O₂ are placed in an evacuated 1.00–liter flask, the reaction represented below occurs.

2SO_{2 (g)} + O_{2 (g)} ↔ 2SO_{3 (g)}

After the reactants and the product reach equilibrium and the initial temperature is restored, the flask is found to contain 0.30 mole of SO₃. Based on these results, the equilibrium constant, Kc, for the reaction is

• 20

• 10

• 6.7

• 2.0

Tags

NGSS.HS-PS1-7

H_2(g) +I_2(g) ↔ 2HI_(g)

All gases begin with an initial concentration of 2.0 M. Equilibrium is established, and the concentration of HI is known to be 4.8 M. What is the value of the equilibrium constant?

• 1.2

• 2.4

• 32

• 64

Consider the following reaction:

NiO(s) + CO(g) ↔ Ni(s) + CO₂(g)

Kc = 4.0 x 10³ (at 1500 K).

If a mixture of solid nickel (II) oxide and 0.10 M carbon monoxide is allowed to come to equilibrium at 1500 K, what will be the equilibrium concentration of carbon dioxide?

• 0.0 M

• 0.10 M

• 0.05 M

Tags

NGSS.HS-PS1-7

A mixture of 0.10 mol of NO, 0.050 mol of H₂, and 0.10 mol of H₂O is placed into a 1.0-L vessel at 300 K.

At equilibrium, [NO] = 0.062 M.

Determine the equilibrium concentrations of H₂, N₂, and H₂O, then determine Kc.

2 NO(g) + 2 H₂ (g) ↔ N₂(g) + 2 H₂O(g)

• Kc = 670

• Kc = 3.58

• Kc = 0.501

What are [A] and [B]?

• concentration of reactants
• concentration of products
• energy of reactants
• energy of products

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6

Which statement correctly describes the potential energy diagram pictured?

• Both forward and reverse reactions are endothermic.

• Both forward and reverse reactions are exothermic.

• The forward reaction is endothermic and the reverse reaction is exothermic.

• The forward reaction is exothermic and the reverse reaction is endothermic.

Tags

NGSS.HS-PS1-4

NGSS.HS-PS3-1