Chemistry Rates of Reaction Revision

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Mindmap of rate of reactions

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Chemistry Rates of Reaction Revision
1 Measuring rates of reaction
1.1 The rate of reaction can be measured by considering the amount of product formed or reactant used in a given period of time
1.2 The rate of reaction changes depending on how far through the reaction is!
1.3 The activation energy is the minimum amount of energy needed for a reaction to occur.
1.4 Gas produced? measure with gas syringe, burette or upside down measuring cylinder
1.4.1 Solid produced? measure with balance
2 The rate of an equation decreases with time. This is because the reactants are used up, resulting in fewer collisions.
3 The rate of reaction increases if the temperature is raised. This is because:
3.1 The reactant particles move more quickly, they have more kinetic energy
3.1.1 This means they move faster, which increases collision frequency More collisions=faster reaction rate
4 Rate of reaction increases if pressure or concentration is increased.
4.1 Particles become more crowded, so collisions are more frequent
4.1.1 Rate of reaction increases.
5 Increasing the concentration of a reactant increases the rate of reaction.
5.1 Reactant particles become more crowded and there is a greater chance of collision.
6 rate of reaction = amount of reactant used or product formed
7 Surface area increases the rate of reaction.
7.1 More particles are exposed to the reactant.
7.1.1 Greater chance of collision, rate increases.
8 Catalysts increase the rate of reaction without being used up.
8.1 They lower the activation energy needed, so more collisions result in a reaction.
8.1.1 Lower costs - less energy is needed.
9 The rate of reaction is the speed at which a reaction happens.
10 Collision theory - reactant particles must collide with activation energy for reaction to occur.
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