The initial rate of a reaction. CIO_2 + OH^- rightarrow products, was measured f
ID: 1009368 • Letter: T
Question
The initial rate of a reaction. CIO_2 + OH^- rightarrow products, was measured for several different starting concentrations of A and B. The following table summarizes the results. Using the data, determine the rate law for the reaction, (answer must be justified using an appropriate method) l/sing data from fine of the experiments above, calculate the magnitude of the rate constant (be sure to assign the correct units to your answer) The first-order rate constant for the decomposition of N_2O_5 to NO_2 and O_2 is 6.8 times 10^-3 s^-1. How much time must elapse for the concentration to decrease to 85 percent of its initial value?Explanation / Answer
order w.r.t ClO2-
(0.01/0.02)^n = (0.0003/0.0012)
n = 2
order w.r.t OH-
(0.012/0.036)^n = (0.0003/0.0009)
n = 1
A) rate law
rate = k[ClO2-]^2[OH-]
B)
rate constant k =
0.0003 = k(0.01^2*0.012)
k = 250 M-2.S-1
2. K = 1/t ln(a/a-x)
6.8*10^-3 = (1/t)ln(100/85)
t = 23.9 sec
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