Identify and describe two factors that increase reaction rates.
1) Temperature: Increasing the temperature of a reaction generally increases the reaction rate. This is because temperature is a measure of the average kinetic energy of the particles involved in the reaction. When the temperature is increased, the kinetic energy of the particles also increases, leading to more frequent and energetic collisions between reactant molecules. These collisions are more likely to have sufficient energy to overcome the activation energy, which is the minimum energy required for a reaction to occur. Therefore, an increase in temperature results in more successful collisions and a faster reaction rate.
2) Concentration or Pressure: Increasing the concentration of reactants in a solution or the pressure of reactant gases increases the reaction rate. This is because a higher concentration or pressure means there are more reactant particles in a given volume, resulting in a greater chance of successful collisions. In a solution, increasing the concentration increases the number of reactant molecules per unit volume, increasing the likelihood of collisions. In the case of gases, as the pressure increases, the gas molecules are closer together, leading to more frequent collisions. Similarly, increasing the pressure of a gas increases the likelihood of successful collisions between gas molecules and a solid or liquid reactant that may be present. Overall, increasing the concentration or pressure increases the frequency of collisions between reactant molecules, leading to an increased reaction rate.