Kinetics (AS)

• The pressure of reactants is another factor that affects reaction rate, as a higher pressure generally leads to a higher reaction rate.
• Increasing the concentration of reactants increases the probability of collisions between molecules, leading to more successful collisions and faster reactions.
• Catalysts are substances that increase the rate of chemical reactions without being consumed themselves. They also provide an alternate pathway.
• Activation energy is the minimum amount of energy required for a reaction to occur.
• A catalyst lowers the activation energy needed for a reaction to take place, allowing it to proceed at a faster rate.
• A catalyst lowers the activation energy by providing an alternative pathway with a lower activation energy.
• Temperature has a significant effect on reaction rates, with most reactions increasing in speed as temperature rises.
• At high temperatures, there are more frequent collisions between particles, resulting in more successful collisions and increased reaction rates.
• Increasing concentration increases the number of reactant molecules available for collision, leading to higher reaction rates.
• Rate of reaction is change in concentration per unit time.
• The peak of the Maxwell Boltzmann Distribution curve shows the most probable energy level of a particle.
• The area under the curve gives the number of particles in an energy range.
• Area under the line from Ea shows the number of particles that could react.
• Homogenous catalysts are in the same phase as the reactants and will often react to produce an intermediate.
• Heterogeneous catalysts are in a different phase to the reactants, commonly as solids.