Problem: The reaction A =&gt; B + C is second order in A. When the initial [A] = 0.100 M, the reaction is 20.0% complete in 26.2 minutes. Calculate the value of the rate constant (in L/min·mol).A. 6.54x10-2B. 9.54x10-5C. 1.52D. 9.54x10-2E. 4.40

FREE Expert Solution

We’re being asked to calculate the value of the rate constant (in L/min•mol) for the reaction below if the reaction is 20.0 =% complete in 26.2%

A → B + C

The integrated rate law for a second-order reaction is as follows:

$\overline{)\frac{\mathbf{1}}{{\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{\mathbf{t}}}{\mathbf{=}}{\mathbf{kt}}{\mathbf{+}}\frac{\mathbf{1}}{{\mathbf{\left[}\mathbf{A}\mathbf{\right]}}_{\mathbf{0}}}}$

where:

[A]t = concentration at time t

k = rate constant

t = time (unknown)

[A]0 = initial concentration

Problem Details

The reaction A => B + C is second order in A. When the initial [A] = 0.100 M, the reaction is 20.0% complete in 26.2 minutes. Calculate the value of the rate constant (in L/min·mol).

A. 6.54x10-2
B. 9.54x10-5
C. 1.52
D. 9.54x10-2
E. 4.40