General Equilibrium

Which of the following expressions is the correct equilibrium-constant expression for the equilibrium between dinitrogen tetroxide and nitrogen dioxide?

N₂O₄ (g) ↔ 2NO₂ (g)

• [NO₂]²

  [N₂O₄]

• [NO₂]

  [N₂O₄]²

• [NO₂][N₂O₄]

• [NO₂]²[N₂O₄]

At equilibrium, ________.

• all chemical reactions have ceased

• the rate constants of the forward and reverse reactions are equal

• the rates of the forward and reverse reactions are equal

• the value of the equilibrium constant is 1

Which one of the following will change the value of an equilibrium constant?

• changing the volume of the reaction vessel

• changing temperature

• varying the initial concentrations of reactants

• adding other substances that do not react with any of the species involved in the equilibrium

The equilibrium expression for Kp for the reaction below is ________.

2O₃ (g) ↔ 3O₂ (g)

• 3(P_O2)

  2(P_O3)

• (P_O2)³

  (P_O3)²

• 2P_O3

  3P_O2

• (P_O3)²

  (P_O2)²

The Keq for the equilibrium below is 7.52 × 10^-2 at 480.0 °C.

2Cl₂ (g) + 2H₂O (g) ↔ 4HCl (g) + O₂ (g)

What is the value of Keq at this temperature for the following reaction?

2HCl (g) + ½O₂ (g) ↔ Cl₂ (g) + H₂O (g)

• -0.0376

• 5.66 × 10-3

• 0.274

• 3.65

Tags

NGSS.HS-PS1-5

The Keq for the equilibrium below is 0.112 at 700.0 °C.

SO₂ (g) + ½O₂ (g) ↔ SO₃ (g)

What is the value of Keq at this temperature for the following reaction?

SO₃ (g) ↔ SO₂ (g) + ½O₂ (g)

• 0.0125

• -0.112

• 8.93

• 0.224

Tags

NGSS.HS-PS1-7

Given the following reaction at equilibrium, if Kc = 1.90 × 10¹⁹ at 25.0 °C, Kp = ________.

H₂ (g) + Br₂ (g) ↔ 2 HBr (g)

• 1.90 × 10¹⁹

• 6.44 × 10⁵

• 1.56 × 10⁴

• 5.26 × 10^-20

Tags

NGSS.HS-PS1-6

Which of the following expressions is the correct equilibrium-constant expression for the reaction below?

CO₂ (s) + H₂O (l)↔ H⁺ (aq) + HCO₃^- (aq)

• [H+][HCO₃^-]

• [H⁺][HCO₃^-] / [CO₂]

• [CO₂][H₂O] / [H⁺][HCO₃^-]

• [CO₂] / [H⁺][HCO₃^-]

The expression for Kp for the reaction below is ________.

4CuO (s) + CH₄ (g) ↔ CO₂ (g) + 4Cu (s) + 2H₂O (g)

• (P_CO2)(P_H2O)²

  (P_CuO)

• [Cu](P_CO2)(P_H2O)²

  [CuO]⁴ (P_CH4)

• (P_CH4)

  (P_H2O)²(P_CO2)

• (P_CO2) (P_H2O)²

  (P_CH4)

Tags

NGSS.HS-PS1-6

The equilibrium constant for the gas phase reaction

N₂ (g) + 3H₂ (g) ↔ 2NH₃ (g)

is Keq = 4.34 × 10^-3 at 300 °C. At equilibrium, ________.

• products predominate (favored)

• reactants predominate (favored)

• roughly equal amounts of products and reactants are present

• only products are present

Tags

NGSS.HS-PS1-6