1.5 Kinetics

• Kinetics is the study of rates of reaction, including how fast things go, how particles move, and how often they collide.
• Rate is the change in concentration or the amount of a reactant or product per unit time.
• Particles can move all the time and they do constantly, unless they are at Absolute Zero.
• Most collisions don't actually lead to a reaction and when they hit off each other they just bounce off each other.
• Activation energy is the minimum amount of energy required for a reaction to occur.
• Activation energy is the energy that's needed, the minimum outlet kinetic energy needed for a reaction to actually happen.
• The most likely energy of a particle in a sample is represented by the peak of the curve.
• The rate of reaction is temperature-dependent, with more particles having more kinetic energy when heated.
• The activation energy is represented by the section of the curve where it crosses the x-axis.
• Particles with energy greater than the activation energy can react, producing products.
• The area under the curve is equal to the total number of molecules.
• The mode is different from the mean.
• A small increase in temperature can lead to a large increase in rates.
• Concentration also affects the rate of reaction, with more frequent collisions and more energetic collisions leading to a faster rate of reaction.
• Activation energy is not for collisions, it's for an actual reaction.
• Activation energy is the difference between the reactants and the top of the reaction profile line.
• Reactions that have a low activation energy need less energy to break them and obviously require less heat energy as well.
• Reactions that have a higher activation energy require lots of energy.
• The Maxwell Boltzmann distribution shows the energy in gas particles, including how often they move and how fast they move.
• Particles in a gas sample move at different speeds, some move slowly and some move quickly, and they have different amounts of kinetic energy.
• The Maxwell Boltzmann plot can be used to display the energy in gas particles.
• Catalysts are substances which increase the rate of reaction by providing an alternative pathway with a lower activation energy.
• Concentration affects the rate of reaction by increasing the likelihood of particles colliding and reacting.
• The rate of reaction can be measured in experiments by the time it takes for a precipitate to form, the amount of mass loss, or the volume of gas produced.
• The Maxwell Boltzmann plot always starts at zero because no particles have zero kinetic energy.