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Questions and Answers
What is the rate of reaction equivalent to?
What does the overall order of a reaction depend on?
What is the unit of the rate constant in a zero-order reaction?
What is the characteristic of a first-order reaction?
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What is the half-life of a first-order reaction dependent on?
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What is necessary for a reaction to occur, according to the Kinetic-Molecular theory?
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What is the minimum energy required for a chemical reaction to occur?
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What is the effect of increasing temperature on the reaction rate?
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What is the purpose of a catalyst in a chemical reaction?
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What is the role of the transition state in a chemical reaction?
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What is the characteristic of an elementary process in a reaction mechanism?
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What is the significance of the rate-determining step in a reaction mechanism?
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Study Notes
Chemical Reaction Basics
- Activation energy is the minimum energy required for a chemical reaction to occur.
- High activation barrier means only a few molecules have sufficient kinetic energy, resulting in a slower reaction.
- Temperature increase leads to an increase in reaction rate.
Transition State and Arrhenius Equation
- The transition state is a hypothetical species between reactants and products on a reaction profile.
- The Arrhenius equation shows that the rate constant increases with increasing temperature and decreasing activation energy.
- The equation is: k = Ae^-Ea/RT, and ln k = (-Ea/RT) + ln A.
Reaction Mechanism
- A reaction mechanism is a step-by-step description of a chemical reaction.
- Each step is an elementary process, and the mechanism must be consistent with stoichiometry and experimentally determined rate law.
- Elementary processes can be unimolecular or bimolecular, and are reversible.
Catalysis
- Catalysis is an alternative reaction pathway with lower energy.
- It increases the rate of reaction, reduces activation energy, and completes the reaction in less time.
Rate of Reaction
- Rate of reaction = ΔM / Δt, where ΔM is the change in concentration of products.
- Rate of reaction = rate of disappearance of reactants = rate of appearance of products.
Rate Law
- The rate law is Rate = k [A]^m [B]^n, where k is the rate constant.
- The overall order of reaction = m + n +…, and m and n are not related to a and b.
Types of Rate Laws
- Zero-Order Rate Law: Rate = k, where the sum of exponents is 0.
- First-Order Rate Law: Rate = k [A], where the sum of exponents is 1.
- Second-Order Rate Law: Rate = k [A]^2, where the sum of exponents is 2.
Half-Life
- The half-life (t½) is the time taken for one-half of a reactant to be consumed.
- For a first-order reaction, the half-life is constant and independent of initial concentration.
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Description
Test your understanding of rates of reaction, rate laws, and the factors that affect them. This quiz covers the concepts of rate of formation, rate of reaction, and rate constant, including zero-order rate laws and how they are affected by temperature, concentration, and catalysts.
