Practice Quiz

1. 1The following mechanism was proposed for a reaction between A and B.
   Step 1: 2A(g) + B(g) <=> C(g) fast
   Step 2: B(g) + C(g) → D(g) slow
   Overall: 2A(g) + 2B(g) → D(g)
   What is the rate law for the overall reaction based on the proposed mechanism?

   1. ARate = k(overall) [A]^2[B]^2
   2. BRate = k(overall) [A][B]^2[C]
   3. CRate = k(overall) [A][B][C]
   4. DRate = k(overall) [A]^2[B]
2. 2For the reaction A → products, successive half-lives are observed to be 10.0 min and 40.0 min. The reaction follows the integrated rate law...

   1. A[A] = -kt + [A]0
   2. Bln[A] = kt + ln[A]0
   3. C1/[A] = kt + 1/[A]0
   4. D1/[A]^2 = kt +1/[A]0^2
3. 3Consider the following reversible reaction. In a 3.00 L container, the following concentrations are found in equilibrium at 400°C: 0.014M N2, 0.172M H2, and 0.0117M NH3. Evaluate Kc.
   N2(g) + 3H2 <=> 2NH3

   1. A0.202
   2. B16.0
   3. C1.99
   4. D4.94
4. 4The conventional equilibrium constant expression (Kc) for the system below is:
   2ICl (s) <=> I2 (s) + Cl2 (g)

   1. AKc = [I2][Cl2] / [ICl]^2
   2. BKc = [Cl2]
   3. CKc = [I2][Cl2] / 2[ICl]^2
   4. DKc = [Cl2] / [ICl]^2
5. 5The reaction for the Haber-Bosch process to produce ammonia in large quantities is:
   N2 (g) + 3H2 (g) <=> 2NH3 (g) K = 4.34 x 10^-3 at 300°C
   What will happen to the equilibrium if a catalyst is added to the reaction system?

   1. AThe equilibrium will shift toward the reactants because the catalyst promotes the reverse reaction over the forward reaction
   2. BThe equilibrium will not change since a catalyst does not affect the equilibrium of a system
   3. CThe equilibrium will shift to the products because there are fewer moles of gas on the right side of the reaction arrow
   4. DThe equilibrium will shift toward the products because the reaction is taking place faster
6. 6When two reactions are added together, how does the expression for the equilibrium constant of the sum reaction (K3) relate to the expression for the equilibrium constants of the original reactions (K1 and K2)?
   A <=> B K1
   B <=> C K2
   ---------------------------------
   A <=> C K3

   1. AK3 = K1 - K2
   2. BK3 = K1 x K2
   3. CK3 = K1 / K2
   4. DK3 = K1 + K2
7. 7The decomposition of ozone may occur through the two-step mechanism shown:
   Step 1: O3 → O2 + O
   Step 2: O3 + O → 2O2
   The oxygen atom is considered to be a(n)...

   1. AReactant
   2. BProduct
   3. CCatalyst
   4. DReaction intermediate
8. 8The following questions refer to the reaction 2A2 + B2 → 2C. The following mechanism has been proposed:
   Step 1 (very slow): A2 + B2 → R + C
   Step 2 (slow): A2 + R → C
   What is the molecularity of step 2?

   1. AUnimolecular
   2. BBimolecular
   3. CTermolecular
9. 9(Part 2 of question 8) Which step is rate determining?
   Step 1 (very slow) A2 + B2 → R + C
   Step 2 (slow) A2 + R → C

   1. ABoth steps
   2. BStep 1
   3. CStep 2
10. 10Name the four important factors which affect the rates of chemical reactions:
    1. [blank_start]Concentrations of reactants[blank_end]
    2. [blank_start]Surface area of solid reactant/catalyst[blank_end]
    3. [blank_start]Temperature of the reaction[blank_end]
    4. [blank_start]The pressure of a catalyst[blank_end]

    1. AConcentrations of reactants
    2. BSurface area of solid reactant/catalyst
    3. CTemperature of the reaction
    4. DPressure of a catalyst

11. 11State the Henderson-Hasselbach equation: [blank_start]pH = pKa + log (HA / A-)[blank_end]

    1. ApH = pKa + log (HA / A-)

Description

Quiz with questions taken from the take-home test.

Author

Kristen Wislowski

Language

English

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6

Tags

chemistrychapter 13: chemical kinetics

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