University:
Georgia Southern University
Course:
CHEM 1310 | Comprehensive General Chemistry
Academic year:

2024
Views:

144

Pages:

2
Author:

Jalen W.

Kinetics Practice Problems 1: a) Write a balanced reaction for which the following rate relationships are true. 𝑅𝑎𝑡𝑒 = − ∆[𝑆2 𝑂8 ] ∆𝑡 =− 1 ∆[𝐼− ] 3 ∆𝑡 = 1 ∆[𝑆𝑂42− ] 2 ∆𝑡 = ∆[𝐼3− ] ∆𝑡 b) If the rate of I- loss is 4.84 × 10-2 M/s, what is the rate of formation of I3-? 2: Given the data in the table, [S2O82⁻]i (M) 0.30 0.44 0.44 a) Initial Rate (M-1s-1) 4.54 6.65 3.33 [I⁻]i (M) 0.42 0.42 0.21 Determine the rate law for the reaction. b) Determine the value for k for the reaction. c) Determine the units on k. d) What is the overall reaction order? 3. The first-order reaction, 2 N2O(g) → 2 N2(g) + O2(g), has a rate constant equal to 0.76 s-1 at 1000 K. How long will it take for the concentration of N2O to decrease to 12% of its initial concentration? 4. Given the following proposed mechanism, predict the rate law for the overall reaction. A2 + 2B → 2AB (overall reaction) Mechanism A2 ⇌ 2A A + B → AB fast slow 5. A first-order reaction has a rate constant of 1.35 × 102 s-1 at 25.0°C. What is the magnitude of k at 95.0°C if Ea = 55.3 kJ/mol? 6. The first-order decomposition of N2O5 at 328 K has a rate constant of 1.70 × 10-3 s-1. If the initial concentration of N2O5 is 2.88 M, what is the concentration of N2O5 after 12.5 minutes? 7. The second-order reaction 2 Mn(CO)5 → Mn2(CO)10, has a rate constant equal to 3.0 × 109 M-1 s-1 at 25°C. If the initial concentration of Mn(CO)5 is 2.0 × 10-5 M, how long will it take for 90.0% of the reactant to disappear? Answers: 1) S2O82⁻(aq) + 3 I⁻(aq) → 2 SO42⁻(g) + I3⁻(aq) 9.68 × 10-2 M/s 2) Rate = 36 M-1s-1 [S2O82⁻][I⁻] second order overall 3) 2.8 s 4) Rate = k [A2]1/2[B] 5) 9.56 × 103 s-1 6) 0.805 M 7) 1.5 × 10-4 s