Consider the following hypothetical aqueous reaction A(aq) rightarrow B(aq). A f

Question

Consider the following hypothetical aqueous reaction A(aq) rightarrow B(aq). A flask is charged with 0.065 mol of A in a total Volume of 100.0 rriL. The following data are collected. Find whether the reaction is first or second order kinetics and calculate the rate constant. Chose the best answer below for the reaction. The reaction is second order and the rate constant is 0.020 M^-1 min^-1. The reaction is second order and the rate constant is 0.040 M^-1 min^-1. The reaction is first order and the rate constant is 0.020 min^-1 The reaction is not of first order, and nor of second order. The reaction is first order and the rate constant is 0.040 min^-1

Explanation / Answer

rate = - d[A] / dt

rate = -(0.051- 0.065) / 10 min

rate = 1.4*10^-3 M/min

the - sign is there because [A] is decreasing.

For second order reaction:

rate [A] ^2
rate = k x [A]^2

rate constant k = rate / [A]^2

k= 1.4*10^-3 / (0.065)^2

k=0.33 /Min M

For first order reaction:

rate [A]
rate = k x [A]

rate constant k = rate / [A]

k= 1.4*10^-3 / (0.065)

k=0.022 /Min

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