Chemistry II - Chemical Equilibrium

The reaction will shift in the direction of products.

Consider the following reaction at equilibrium. What effect will adding more H2S have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

The reaction will shift to the left in the direction of reactants.

Consider the following reaction at equilibrium. What effect will increasing the volume of the reaction mixture have on the system? 2 H2S(g) + 3 O2(g) ⇌ 2 H2O(g) + 2 SO2(g)

The reaction will shift in the direction of reactants.

Consider the following reaction at equilibrium. What effect will removing NO2 have on the system? SO2(g) + NO2(g) ⇌ SO3(g) + NO(g)

No change in equilibrium is observed.

Consider the following reaction at equilibrium. What will happen if FeS2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g)

The equilibrium will change in the direction of the products.

Consider the following reaction at equilibrium. What will happen if O2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g)

The equilibrium will change in the direction of the reactants.

Consider the following reaction at equilibrium. What will happen if SO2 is added to the reaction? 4 FeS2(s) + 11 O2(g) ⇌ 2 Fe2O3(s) + 8 SO2(g)

When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance.

Define Le Chatelier's Principle.

the rate of the forward reaction equals the rate of the reverse reaction

Define dynamic equilibrium.

K = [NH3]^20 / [N2]^10 [H2]^30

Express the equilibrium constant for the following reaction. 10 N2(g) + 30 H2(g) ⇔ 20 NH3(g)

K = [N2]^6 [H2]^18 / [NH3]^12

Express the equilibrium constant for the following reaction. 12 NH3(g) ⇔ 6 N2(g) + 18 H2(g)

K = [CH2Cl2]^4 [H2]^2 / [CH3Cl]^4 [Cl2]^2

Express the equilibrium constant for the following reaction. 4 CH3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)

K = [HBr]^16 / [H2]^8 [Br2]^8

Express the equilibrium constant for the following reaction. 8 H2(g) + 8 Br2(g) ⇌ 16 HBr(g)

K = [CO2] [H2O]^2 / [CH4] [O2]^2

Express the equilibrium constant for the following reaction. CH4(g) + 2 O2(g) ⇔ CO2(g) + 2 H2O(g)

K = [CH3Cl]^4 [Cl2]^2 / [CH2Cl2]^4 [H2]^2

Express the reverse equilibrium constant for the following reaction. 4 CH3Cl(g) + 2 Cl2(g) ⇔ 4 CH2Cl2(g) + 2 H2(g)

K = [H2]^8 [Br2]^8 / [Hbr]^16

Express the reverse equilibrium constant for the following reaction. 8 H2(g) + 8 Br2(g) ⇌ 16 HBr(g)

The reverse reaction is favored.

Give the direction of the reaction, if K << 1.

The forward reaction is favored.

Give the direction of the reaction, if K >> 1. - The forward reaction is favored. - The reverse reaction is favored. - Neither direction is favored. - If the temperature is raised, then the forward reaction is favored. - If the temperature is raised, then the reverse reaction is favored.

Neither direction is favored.

Give the direction of the reaction, if K ≈ 1.

oxygen

Hemoglobin carries ________ in the blood.

∞

In a reaction mixture containing only products, what is the value of Q?

0

In a reaction mixture containing only reactants, what is the value of Q?

1

In a reaction mixture containing reactants and products, each at a concentration of 1M, what is the value of Q?

SO3(g) + NO(g) ⇌ SO2(g) + NO2(g)

In which of the following reactions will Kc = Kp? - 4 NH3(g) + 3 O2(g) ⇌ 2 N2(g) + 6 H2O(g) - 2 SO2(g) + O2(g) ⇌ 2 SO3(g) - SO3(g) + NO(g) ⇌ SO2(g) + NO2(g) - 2 N2(g) + O2(g) ⇌ 2 N2O(g) - None of the above reactions have Kc = Kp.

2.6 × 10-5

The equilibrium constant is given for one of the reactions below. Determine the value of the missing equilibrium constant. H2(g) + Br2(g) ⇌ HBr(g) Kc = 3.8 × 104 HBr(g) ⇌ H2(g) + Br2(g) Kc = ?

removing O2 raising the temperature adding SO3 (all of the above)

The following reaction is exothermic. Which change will shift the equilibrium to the left? 2 SO2(g) + O2(g) ⇌ 2 SO3(g)

K >> 1 implies that the reaction is very fast at producing products.

Which of the following statements is FALSE? - K >> 1 implies that the reaction is very fast at producing products. - When K >> 1, the forward reaction is favored and essentially goes to completion. - When K << 1, the reverse reaction is favored and the forward reaction does not proceed to a great extent. - When K ≈ 1, neither the forward or reverse reaction is strongly favored, and about the same amount of reactants and products exist at equilibrium. - None of the above.

If Q = K, it means the reaction is at equilibrium

Which of the following statements is TRUE? - If Q = K, it means the reaction is at equilibrium. - If Q < K, it means the reverse reaction will proceed to form more reactants. - If Q > K, it means the forward reaction will proceed to form more products. - All of the above are true. - None of the above are true.

If Q < K, it means the forward reaction will proceed to form more products.

Which of the following statements is TRUE? - If Q = K, it means the reaction is not at equilibrium. - If Q < K, it means the forward reaction will proceed to form more products. - If Q > K, it means the forward reaction will proceed to form more products. - All of the above are true. - None of the above is true.

If Q > K, it means the reverse reaction will proceed to form more reactants.

Which of the following statements is TRUE? - If Q > K, it means the reverse reaction will proceed to form more reactants. - If Q < K, it means the reverse reaction will proceed to form more reactants. - If Q = K, it means the reaction is not at equilibrium. - All of the above are true. - None of the above are true.

Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, measured at any point in the reaction

Which of the following statements is TRUE? - Reaction quotient is the concentration of the reactants raised to the stoichiometric coefficients divided by the concentration of the products raised to their stoichiometric coefficients, measured at any point in the reaction. - Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, measured at any point in the reaction. - Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, measured at equilibrium. - Reaction quotient is the concentration of the reactants raised to the stoichiometric coefficients divided by the concentration of the products raised to their stoichiometric coefficients, measured at equilibrium. - Reaction quotient is the concentration of the products raised to the stoichiometric coefficients divided by the concentration of the reactants raised to their stoichiometric coefficients, at the point both are equal.