Table of Contents

 

AQA | Unit 1 | Chemistry 1

Page 1 | Atoms, periodic table, chemical reactions

Page 2 | Limestone and Building Materials

Page 3 | Metal and their uses

Page 4 | Crude oil and fuels

Page 5 | Other useful substances from crude oil

Page 6 | Plant oils and their uses

Page 7 | Changes in the earth and its atmosphere

AQA | Unit 2 | Chemistry 2

Page 1 | Structure and Bonding 

 Page 2  | Atomic structure, analysis and quantitative chemistry

Page 3 | Rates of Reactions

Page 4 | Exothermic and Endothermic Reaction

Page 5 | Acids, Bases and Salts

Page 6 | Electrolysis

AQA | Unit 3 | Chemistry 3

Page 1 | The periodic table

Page 2 | Water

Page 3 | Calculating and explaining energy change

Page 4 | Further analysis and quantitative chemistry

Page 5 | The production of ammonia

Page 6 | Alcohols, carboxylic acids and esters

 

Rates of Reaction


Learning objectives:

to learn how reactions can be measured, and what can affect the speed of reactions 

Different reactions occur at different rates. There are different ways to measure the rate of a reaction

⦁ Measure the rate at which the reactant is used up

⦁ Measure the rate at which the product is used up

When measuring the rate of reaction, we can measure many things.

⦁ we can measure the mas of a substance and see how much it changes

 ⦁ we can measure the volume of gas and see how much Is produced over a period of time

the rate of reaction is measured using this equation

Factors affecting the rate

The rate of reaction can be affected by a number of factors

⦁ Temperature
⦁ Concentration of reactant
⦁ Pressure
⦁ Surface area
⦁ Catalyst

If the temperature increases or decreases then the rate of reaction will change
This graph will illustrate the changes produced by different temperatures

collision Theory

 

Collision theory


For the chemical reaction to occur the reactant particles must collide. However the collisions must occur with enough energy for the reaction to occur.

Pressure – if the pressure or concentration is increased then there are more particles in a particular volume.
Therefore if the pressure is increases then there is a greater chance of the particles colliding and the rate of the reaction increases.

Increase in pressure

 

Surface area – if a solid reactant is broken down into little pieces the surface area increase as there are more particles exposed to the other reactant, therefore increasing the chance of the particles colliding and thus the rate of reaction increases

Changing the temperature – if the temperature is increased, the reactant particles move more quickly and collude with greater energy, therefore they have enough energy to get over the activation energy. The activation energy is the minimum amount of energy required for the reaction to occur.

Using a catalyst – catalyst increase the rate of reaction by lowering the activation energy so more of the collisions are likely to be successful. The key about using a catalyst is that it does not used up in the reaction and remains chemically unchanged.

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