Equilibrium Constant

An equilibrium constant with a value K > 1 means:

• a. there are more reactants than products at equilibrium
• b. there are more products than reactants at equilibrium
• c. there are the same amount of products and reactants at equilibrium
• d. the reaction is not at equilibrium

Tags

NGSS.HS-PS1-6

Equal amounts of reactants are poured into a suitable container. Given sufficient time, the reactants may be converted almost entirely to products if:

• a. K is less than 1
• b. K is greater than 1
• c. K is equal to 1
• d. K is equal to 0

Tags

NGSS.HS-PS1-6

The equilibrium constant for the reaction H2 (g) + I2 (g) ↔ 2 HI (g) would be

• a. K = [HI]2/[H2][I2]
• b. K = [H2][I2]/[HI]2
• c. K = 2[HI]/[H2][I2]
• d. K = [H2][I2]/2[HI]

The equilibrium constant for the reaction 2 SO2 (g) + O2 (g) ↔ 2 SO3 (g) would be

• a. K = 2[SO3]/2[SO2][O2]
• b. K = 2[SO2][O2]/[SO3]
• c. K = [SO3]2/[SO2]2[O2]
• d. K = [SO2]2[O2]/[SO3]2

Tags

NGSS.HS-PS1-7

The equilibrium constant for the reaction Ca(HCO3)2 (s) ↔ CaO (s) + 2 CO2 (g) + H2O (g) would be

• a. K = [CaO][CO2]2[H2O]/[Ca(HCO3)2]
• b. K = [Ca(HCO3)2]/[CaO][CO2]2[H2O]
• c. K = [CO2]2
• d. K = [CO2]2[H2O]

The equilibrium constant for the reaction SnO2 (s) + 2 H2 (g) ↔ Sn (s) + 2 H2O (g) would be

• a. K = [H2O]2/[H2]2
• b. K = [Sn][H2O]2/[SnO][H2]2
• c. K = [SnO][H2]2/[Sn][H2O]2
• d. K = [H2]2/[H2O]2

Tags

NGSS.HS-PS1-7

For the reaction H2 (g) + Br2 (g) ↔ 2 HBr (g), K = 4.0 x 10-2. For the reaction 2 HBr (g) ↔ H2 (g) + Br2 (g) K =:

• a. 4.0 x 10-2
• b. 5
• c. 25
• d. 2.0 x 10-1

At a certain temperature, K = 1 for the reaction. At equilibrium, you can be certain that:

• a. [H2] = [Cl2]
• b. [HCl] = 2[H2]
• c. [HCl] = [H2] = [Cl2] = 1
• d. [H2][Cl2]/[HCl]2 = 1

For the reaction: A + B ↔ C + D 6.0 moles of A and 5.0 moles of B are mixed together in a suitable container. When equilibrium is reached, 4.0 moles of C are produced. The equilibrium constant for this reaction is:

• a. K = 1/8
• b. K = 8
• c. K = 30/16
• d. K = 16/30

Tags

NGSS.HS-PS1-7

The Haber process is a method to produce ammonia from hydrogen and nitrogen gasses. The reaction is N2 (g) + 3 H2 (g) ↔ 2 NH3 (g) If hydrogen gas is added after the reaction has reached equilibrium, the reaction will:

• a. shift to the right to produce more product
• b. shift to the left to produce more reactants
• c. stop. All the nitrogen gas has already been used up.
• d. Need more information.

Tags

NGSS.HS-PS1-5

NGSS.HS-PS1-6