Chapter 15, Problem 131CP

Consider the hypothetical reaction

$\text{A}\text{+}\text{B}\text{+}2\text{C}\to \text{2D}\text{+}\text{3E}$

In a study of this reaction, three experiments were run at the same temperature. The rate is defined as $-\text{d[B]/dt}$ .

$\text{Experiment}\text{1:}$

${\text{[A]}}_{\text{0}}=2.0\text{M}{\text{[B]}}_0=1.0\times {10}^{-3}\text{M}{\text{[C]}}_0=1.0\text{M}$

$\text{Experiment}2\text{:}$

${\text{[A]}}_{\text{0}}=1.0\times {10}^{-2}\text{M}{\text{[B]}}_0=3.0\text{M}{\text{[C]}}_0=1.0\text{M}$

$\text{Experiment}3\text{:}$

${\text{[A]}}_{\text{0}}=10.0\text{M}{\text{[B]}}_0=5.0\text{M}{\text{[C]}}_0=5.0\times {10}^{-1}\text{M}$

Write the rate law for this reaction, and calculate the rate constant.