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Questions and Answers
What is chemical kinetics?
What is chemical kinetics?
The branch of chemistry that deals with the study of reaction rates and their mechanisms.
What is the unit of rate of reaction?
What is the unit of rate of reaction?
mol L-1s-1
What is the rate law or rate equation?
What is the rate law or rate equation?
It is an expression that relates the rate of reaction with the concentration of the reactants.
What does molecularity of a reaction refer to?
What does molecularity of a reaction refer to?
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How can the order of a reaction be determined?
How can the order of a reaction be determined?
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What is the half-life of a reaction?
What is the half-life of a reaction?
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What is the Arrhenius equation used for?
What is the Arrhenius equation used for?
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What is a pseudo first order reaction?
What is a pseudo first order reaction?
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Which of the following statements is true regarding rate constants?
Which of the following statements is true regarding rate constants?
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Study Notes
Chemical Kinetics
- Chemical kinetics studies reaction rates and mechanisms.
- Rate of reaction is the change in reactant or product concentration per unit time.
- Units of rate of reaction are mol L-1s-1.
- Rate law relates reaction rate to reactant concentrations.
- Rate constant (k) is the proportionality constant in the rate law.
- Average rate is the rate measured over a long time interval.
- Instantaneous rate is the rate at a specific moment in time.
- Molecularity is the number of reactant molecules involved in a single step of a reaction mechanism.
- Order of reaction is the sum of the exponents of reactant concentrations in the rate law.
- Half-life (t1/2) is the time required for half of the reactant to be consumed.
- Zero order reaction: rate is independent of reactant concentration, t1/2 = [Ro]/2k.
- First order reaction: rate depends linearly on reactant concentration, t1/2 = ln(2)/k.
- Pseudo first order reaction: a bimolecular reaction that behaves like a first order reaction due to one reactant being in excess.
- Activation energy (Ea) is the minimum energy required for reactants to overcome the energy barrier and react.
- Arrhenius equation relates rate constant k to temperature T: k = Ae-Ea/RT.
- Frequency factor (A) represents the frequency of collisions.
- Reaction mechanism is the sequence of elementary steps leading to the overall reaction.
- Activated complex is an unstable intermediate formed during the reaction.
- Rate determining step is the slowest step in the reaction mechanism.
Factors Affecting Rate of Reaction:
- Nature of reactants - Some reactions are faster than others due to inherent properties.
- Concentration of reactants - Higher concentration leads to more collisions, increasing rate.
- Surface area - Increased surface area in heterogeneous reactions offers more contact points, speeding up the process.
- Temperature - Increasing temperature provides more energy for reactions to occur, leading to a faster rate.
- Catalyst - A catalyst lowers activation energy, providing an alternative reaction pathway and speeding up the process.
- Presence of light - Some reactions are initiated by light, such as photochemical reactions.
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Description
Explore the key concepts of chemical kinetics, including reaction rates, rate laws, and molecularity. This quiz covers topics like average and instantaneous rates, order of reaction, and half-life. Test your understanding of these fundamental principles in chemistry.
