Author Question: For the second-order reaction NO(g) + O3(g) NO2(g) + O2(g), the rate constant has been measured to ... (Read 68 times)

Frost2351 · **on:** Mar 21, 2021

Question 1

For the reaction A → Products, successive half-lives are observed to be 10.0 min and 40.0 min. At the beginning of the reaction, [A] was 0.74 M. The numerical value of the rate constant is:

Reference: Ref 12-13

◦ 0.069
◦ 0.14
◦ 10.
◦ 0.037
◦ None of these are correct.

Question 2

For the second-order reaction NO(g) + O₃(g) → NO₂(g) + O₂(g), the rate constant has been measured to be 1.08 × 10⁷M^–1 s^–1 at 298 K and the activation energy has been measured to be 11.4 kJ/mol over the temperature range 195 K to 304 K. What is the rate constant at 243 K? (R = 8.3145 J K^–1 mol^–1)

◦ 1.08 × 10⁷M^–1 s^–1

◦ 1.08 × 10⁹M^–1 s^–1

◦ 3.81 × 10⁶M^–1 s^–1

◦ 3.06 × 10⁷M^–1 s^–1

◦ 9.51 × 10⁵M^–1 s^–1

xoxo123 · **Reply #1 on:** Mar 21, 2021

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