Basics of Reaction Rates
What does the term "reaction rate" mean?
Reaction rate is how fast a reaction happens.
Describe the affect of the surface area on the rate of a chemical reaction.
More surface area makes reactions go faster.
What is the collision theory, and how does it explain the reaction rates?
Collision theory says reactions happen when the particles collide with enough energy and in the right way.
What is a reaction mechanism, and how does it relate to reaction rates?
The reaction mechanism is the step-by-step process of how the reactions happen. Which it affects how fast the reactions go.
Outline a method for experimentally determining the rate of a chemical reaction.
By measuring how fast the reactants disappear or products from over time.
How does the concentration of reactants affect the reaction rate?
More reactants mean a faster reaction.
How does the nature of the reactants influence the reaction rates?
By the different chemicals react at a different speeds.
What is the concept of the effective collisions in the collision theory.
The effectiveness of the collisions are when the particles collide and react.
Explain the term "rate-determining step" in the context of reaction mechanisms.
The rate-determining step is the slowest step in a reaction mechanism, determining on how fast the overall reaction is.
What is a rate law, and how is it determined experimentally?
The rate law shows how reactant concentrations affect the reaction rate. It's found by doing experiments and analyzing the data.
Explain the role of the temperature in influencing the reaction rates.
Higher temperature makes reactions go faster.
Discuss the impact of the pressure on the rate of gas-phase reactions.
Higher the pressure makes the gas reactions faster.
Explain how increasing the temperature affects the collisions frequency and the reaction rates.
Higher temperature means particles move faster, by increasing the collisions and the reaction rates.
What is the difference between elementary reactions and overall reactions.
The elementary reactions are individual steps in a reaction mechanism. Overall reactions show the whole reaction.
Describe how initial rates are used to determine reactions orders.
The initial rates shows how reactants concentrations affect the reaction rates at the beginning. This helps determine reactions orders.
Define activation energy and its significance in the reaction rates.
Activation energy is the energy needed to start a reaction. High activation energy means slower reaction.
Explain the role of solvent in influencing the reaction rates in the solution-phase reactions.
The solvents can speed up the reactions by dissolving reactants.
How does increasing the concentration of the reactants impact collision frequency and reaction rates?
More reactants mean more collisions and faster reaction rates.
How do catalysts influence reaction mechanisms?
The catalysts speeds up the reactions by providing an easier pathway.
What is the significance of the reaction rate constants in the rate equation.
How does the presence of a catalyst affect the rate of a chemical reaction?
Catalysts speeds up the reactions without being used up by themselves.
Describe how the presence of impurities can affect the reaction rates.
The impurities can slow down or speed up its reactions.
Describe the relationship between activation energy and the likelihood of successful collisions.
Higher activation energy means fewer successful collisions.
Describe how intermediates and transition states contribute to reactions mechanisms.
The intermediates are in-between products in a reaction. Transition states are the high-energy points in a reaction. They both affect how fast reactions go.
What is the use of graphical methods, such as the method of initial rates or integrated rate laws, in determining the reaction rates.
The graphs help analyze data to find reactions rates, reactions orders, and rate constants.