Question

1. The initial concentrations of reactants and products for this reaction are given below. N2(g) + O2(g) ⇄ 2NO(g) Calculate Q for this reaction. Answer this to one decimal place (e.g. 10.2) The initial concentration of N2 is 1.0 M The initial concentration of O2 is 1.0 M The initial concentration of NO is 2.5 M

2. The reaction below is not at equilibria and Q = 1.7. The equilibrium constant is K = 0.230. 2SO3(g) ⇌ 2SO2(g) + O2(g) Which direction does the reaction shift to reach equilibria?

- To the left (reactants side) as Q > K meaning the concentrations of products must be increased to reach equilibrium.

- To the left (reactants side) as Q > K meaning the concentrations of products must be reduced to reach equilibrium. .

-To the right (products side) as Q > K meaning the concentrations of products must be increased to reach equilibrium.

-To the right (products side) as Q > K meaning the concentrations of products must be decreased to reach equilibrium.

3. Given the following reaction at equilibrium 2NH3(g) → N2(g) + 3H2(g) ΔH = +92.4 kJ mol-1 choose all of the answers that apply.

-To restore equilibrium, the reaction shifts to the right (products) side when heat is added.

-To restore equilibrium, the reaction shifts to the left (reactants) side when heat is added.

- To restore equilibrium, the reaction shifts to the left (reactants) side when the volume of the reaction container decreases.

- To restore equilibrium, the reaction shifts to the right (products) side when the volume of the reaction container decreases.

- To restore equilibrium, the reaction shifts to the left (reactants) side when the concentration of NH3(g) is reduced.

-To restore equilibrium, the reaction shifts to the right (products) side when the concentration of NH3(g) is reduced.

4. Given the following reaction at equilibrium CaO(s) + CO2(g) ⇌ CaCO3(s) select all of the answers that apply.

-To restore equilibrium, the reaction shifts to the right (products) side when the total pressure of the system is increased.

- To restore equilibrium, the reaction shifts to the left (reactants) side when the total pressure of the system is increased

- To restore equilibrium, the reaction shifts to the left (reactants) side when CaO(s) is added.

- To restore equilibrium, the reaction shifts to the right (products) side when CaO(s) is added.

-To restore equilibrium, the reaction shifts to the right (products) side when CO2 is added.

- To restore equilibrium, the reaction shifts to the left (reactants) side when CO2 is added.

5. Select the correct reaction when H2PO4- (a Bronsted-Lowry acid) reacts with water.

1. H2PO4- + H2O ⇄ OH- + PO43-

2. H2PO4- + H2O ⇄ H3O+ + HPO42-

3. H2PO4- + OH- ⇄ H2O + HPO42-

4. H2PO4- + H2O ⇄ O2- + H4PO4+

6. Select the correct reaction when NH2- (a Bronsted-Lowry base) reacts with water.

1. NH2- + OH- ⇄ NH2- + H3O+

2. NH2- + H3O+ ⇄ NH3 + H2O

3. NH2- + H2O ⇄ NH3 + OH-

4. NH2- + H2O ⇄ NH2- + H3O+

7.

The ionization constant for water (K_w) is 2.9 × 10⁻¹⁴ at 40 °C. Calculate the pH of water at 40^oC.

Enter your answer to one decimal place (10.2).

8. Calculate the pH of a 0.1 M solution of HCl. (HCl is a strong acid that completely ionizes in water.)

Enter your answer to one decimal place (e.g. 2.1). Do not enter units.

9. Calculate the pOH of a 2.0 M solution of Ba(OH)₂.

Enter your answer to one decimal place. Do not enter units.

10. Calculate the equilibrium constant at 25 °C for the weak base (CH₃)₂NH. Its weak acid is (CH₃)₂NH₂⁺ , K_a = 1.7 x 10^-11

Please use decimal notation and use two digits (e.g. 0.0025)

Answer 1

conc. =) Reaction Quotient (0) to calc. the ce , we use initial of mactant and product. N₂ (g) + O₂(g) = 2 No cgi B = I No]? [N,] [O] a = (2.5)2 = 6.25 (1) (1)