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.