Consider the following reaction: 2N_2O(g) rightarrow 2N_2(g) + O_2(g) rate = k[N

Question

Consider the following reaction: 2N_2O(g) rightarrow 2N_2(g) + O_2(g) rate = k[N_2O] For an initial concentration of N_2O of 0.50 M, calculate the concentration of N_2O remaining after 2.0 min if k = 3.4 Times 10^-3 s^-1. 0.17 M 0.66 M 0.33 M 0.55 M 0.50 M Consider the following: 2A rightarrow A_2 rate = k[A]^2 If the rate constant is 1.43 M^-1 s^-1 and the initial concentration of A is 0.0180 M, calculate the time for the rate of consumption of A to drop to 1.25 Times 10^-5 M s^-1. 80.0 s 197 s 236 s 159 s 99.0 s A first-order reaction has a rate constant of 26 s^-1. If the initial concentration of reactant is 0.082 M, how long will it take for the reactant to reach 0.0010 M? 0.074 s 2.2 s 0.097 s 0.038 s 0.17 s A compound decomposes with a half-life of 8.0 s and the half-life is independent of the concentration. How long does it take for the concentration to decrease to one-sixteenth of its initial value? 24 s 32 s 40 s 130 s 64 s

Explanation / Answer

12. (B)

11.

k = (2.303/t)log(a/a-x)

26 = 2.303/t log (0.082/0.001)

t = 0.1686 s

09.

Use equation k = 2.303/t log(a/a-x) to get remaining concentration (a-x)

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