Q16.26P - Chemistry: Molecular Nature Of Matter And Change

Question

Give the individual reaction orders for all substances and the overall reaction order from the following rate law:

$\mathbf{Rate}\mathbf{=}\mathbf{k}\left[{{\mathrm{BrO}}_3}^{-}\right]\left[{\mathrm{Br}}^{-}\right]{\left[H^{+}\right]}^{\mathbf{2}}$

Step-by-Step Solution

Answer

In terms of  $\left[{{\mathrm{BrO}}_3}^{-}\right]$, $\left[{\mathrm{Br}}^{-}\right]$, $\left[{\mathrm{H}}^{+}\right]$   the order is 1, 1, and 2.

And the overall reaction order is 4.

Step 1: Individual reaction orders for all substancesa

To establish the order of each reactant, use the exponent on each concentration term in the rate law.

In terms of  $\left[{{\mathrm{BrO}}_3}^{-}\right]$, the order is 1.

In terms of $\left[{\mathrm{Br}}^{-}\right]$ , the order is 1.

In terms of  $\left[{\mathrm{H}}^{+}\right]$, the order is 2.

Step 2: Overall reaction order

To determine the overall reaction order, add the individual order of reactants:

Overall order = 1+1+2 =4

As a result, the overall reaction order is 4.