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The reaction below has a Kp value of 3.3 × 10-5. What is the value of Kc for this reaction at 700 K? 2 SO3(g) ⇌ 2 SO2(g) + O2(g) A) 5.7 × 10-7 B) 1.7 × 106 C) 3.3 × 10-5 D) 3.0 × 104 E) 1.9 × 10-3

A) 5.7 × 10-7

Give the direction of the reaction, if K >> 1. A) The forward reaction is favored B) The reverse reaction is favored C) Neither direction is favored D) If the temperature is raised, then the forward reaction is favored E) If the temperature is raised, then the reverse reaction is favored

A) The forward reaction is favored

Equilibrium in which rate of the forward reaction equals the rate of the reverse reaction is. A) dynamic B) temperature independent C) concentration independent D) volume independent

A) dynamic

If a chemist wishes to prepare a buffer that will be effective at a pH of 3.00 at 25°C, the best choice would be an acid component with a Ka equal to A) 9.10 × 10-2. B) 9.10 × 10-4. C) 9.10 × 10-6. D) 9.10 × 10-8. E) 9.10 × 10-10.

B) 9.10 × 10-4.

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

B) SO3(g) + NO(g) ⇌ SO2(g) + NO2(g)

Give the direction of the reaction, if K << 1 A) The forward reaction is favored B) The reverse reaction is favored C) Neither direction is favored D) If the temperature is raised, then the forward reaction is favored E) If the temperature is raised, then the reverse reaction is favored.

B) The reverse reaction is favored

Calculate the pH of a solution formed by mixing 250.0 mL of 0.900 M NH4Cl with 250.0 mL of 1.60 M NH3. The Kb for NH3 is 1.8 × 10-5. A) 8.25 B) 9.18 C) 9.50 D) 10.12 E) 10.83

C) 9.50

Give the direction of the reaction, if K ≈ 1 A) The forward reaction is favored B) The reverse reaction is favored C) Neither direction is favored D) If the temperature is raised, then the forward reaction is favored E) If the temperature is raised, then the reverse reaction is favored

C) Neither direction is favored

An important buffer in the blood is a mixture of A) sodium chloride and hydrochloric acid. B) hydrochloric acid and sodium hydroxide. C) carbonic acid and bicarbonate ion. D) acetic acid and bicarbonate ion. E) acetic acid and carbonate ion.

C) carbonic acid and bicarbonate ion

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

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

If the pKa of HCHO2 is 3.74 and the pH of an HCHO2/NaCHO2 solution is 3.11, which of the following is TRUE? A) [HCHO2] < [NaCHO2] B) [HCHO2] = [NaCHO2] C) [HCHO2] << [NaCHO2] D) [HCHO2] > [NaCHO2] E) It is not possible to make a buffer of this pH from HCHO2 and NaCHO2.

D) [HCHO2] > [NaCHO2]

Chemical equilibrium is the result of A) all of the reactants being converted into products B) stoppage of further reaction C) formation of products equal in mass to the mass of the reactants D) opposing reactions attaining equal rates E) a loss of pressure in the system.

D) opposing reactions attaining equal rates

10) The reaction below has a Kc value of 3.64 × 10-3. What is the value of Kp for this reaction at 25°C? 2 NaN3(s) ⇌ 2 Na(s) + 3 N2(g) A) 131 B) 0.613 C) 8.90 × 10-2 D) 29.9 E) 53.2

E) 53.2

Identify a good buffer. A) small amounts of both a weak acid and its conjugate base B) significant amounts of both a strong acid and a strong base C) small amounts of both a strong acid and a strong base D) significant amounts of both a weak acid and a strong acid E) significant amounts of both a weak acid and its conjugate base

E) significant amounts of both a weak acid and its conjugate base

Express the equilibrium constant for the following reaction. 16 CH3Cl(g) + 8 Cl2(g) ⇔ 16 CH2Cl2(g) + 8 H2(g)

K = [CH2Cl2]16[H2]8/[CH3Cl]16[Cl2]8