Rates of Reaction

Andrew Barton
Mind Map by Andrew Barton, updated more than 1 year ago
Andrew Barton
Created by Andrew Barton about 6 years ago


A comprehensive mind map of various factors involved with Rates of Reaction.

Resource summary

Rates of Reaction
  1. The rate of reaction tells us how quickly a chemical reactions happens
    1. Calculation: How much reactant is used up ÷ time it takes to complete the reaction
      1. eg. Amount of hydrogen gas formed (cm3) ÷ Time for reactant to be used up
    2. Effect of Surface Area
      1. Measure of how much surface is exposed
        1. As the surface area is increased, the rate of reaction increases
          1. ex: A block a wood will burn slower than wood shavings as there is less particles to react with on the surface.
            1. Explanation: As the surface area is increased, there are more open particles that can be reacted with
      2. Collision Theory
        1. Before a chemical reaction can start, particles must crash together
          1. The more collisions between particles in a given time, the faster the reaction.
        2. Effect of Temperature
          1. When particles are heated, they gain more thermal energy and they move around quicker.
            1. As they travel faster, there are more collisions in a certain time.
              1. Therefore, reactions get faster as temperature is raised.
                1. Also, some particles when colliding just bounce off each other because they don't have enough energy.
                  1. At higher temperatures, particles are moving faster and they collide with more force, therefore more collisions produce reactions.
                    1. So raising the temperature: 1) Makes particles collide more often in a certain time. 2) Makes it more likely that collisions result in a reactions.
          2. Catalysts
            1. A catalyst is a substance which speed up a chemical reaction. At the end of the reaction, the catalyst is chemically unchanged.
              1. Before reactants can turn into products, they need enough energy to start the reaction.
                1. The energy needed to start a reaction is called its ACTIVATION ENERGY.
                  1. A catalyst LOWERS the activation energy.
                    1. Catalysts make it easier for particles to react as less energy is needed to start a reaction.
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