# Rates of Reaction

Hope it helps!

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• Created by: Hope
• Created on: 19-11-08 16:41
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## Pages in this set

### Page 1

The effect of concentration on rate

Rate of reaction = rate at which reactants are turned into products

For example-

The decomposition of hydrogen peroxide to form water and oxygen.

We could measure the rate or this reaction in the moles of product (H2O or O2) formed per a second…

### Page 2

Oxygen can be collected and measured using an inverted burette.

volume of 02/ cm 3

Time /s

Looking at the graph you can see-
o The graph is steep at first, when the concentration of hydrogen peroxide is highest, before
any has been used up. The rate of reaction at…

### Page 3

Gives the general rate equation rate = k [A]m [B]n

Rate [A]

Order of reaction 0 (zero) with respect to A ­ means no change in the rate of reaction when I change [A]

Order of reaction 1 with respect to A ­ means that if [A] is doubled, then…

### Page 4

mixture at the point t=0, or by using a clock technique to find the reaction time for
a small amount of reaction to take place)
o Half-lives method- By using the progress curve to find half-lives for the
reaction you can see that if the half-lives are constant, the reaction…