Chapter 16: Q16.26P (page 730)

Give the individual reaction orders for all substances and the overall reaction order from the following rate law:
$Rate = k [{BrO}_{3}^{-}] [{Br}^{-}] {[H^{+}]}^{2}$

Short Answer

Expert verified

In terms of $[{BrO}_{3}^{-}]$ , $[{Br}^{-}]$ , $[H^{+}]$ the order is 1, 1, and 2.

And the overall reaction order is 4.

Step by step solution

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 $[{BrO}_{3}^{-}]$ , the order is 1.

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

In terms of $[H^{+}]$ , 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.

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Experiment	Initial $[C S_{2}]$ mol/L	Initial rate ( $m o l / L s^{- 1}$ )
1	0.100	$2.7 \times 10^{- 7}$
2	0.080	2.2 $\times 10^{- 7}$
3	0.055	1.5 $\times 10^{- 7}$
4	0.044	1.2 $\times 10^{- 7}$

Give the individual reaction orders for all substances and the overall reaction order from the following rate law:
$Rate = k [{BrO}_{3}^{-}] [{Br}^{-}] {[H^{+}]}^{2}$

Short Answer

Step by step solution

Individual reaction orders for all substancesa

Step 2: Overall reaction order

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Give the individual reaction orders for all substances and the overall reaction order from the following rate law:Rate=k[BrO3-][Br-][H+]2

Short Answer

Step by step solution

Individual reaction orders for all substancesa

Step 2: Overall reaction order

One App. One Place for Learning.

Most popular questions from this chapter

Recommended explanations on Chemistry Textbooks

Chemical Reactions

Making Measurements

Ionic and Molecular Compounds

Nuclear Chemistry

Kinetics

Organic Chemistry

Study anywhere. Anytime. Across all devices.

Give the individual reaction orders for all substances and the overall reaction order from the following rate law:
$Rate = k [{BrO}_{3}^{-}] [{Br}^{-}] {[H^{+}]}^{2}$