Podcast
Questions and Answers
The bottom of the energy diagram represents the activation complex.
The bottom of the energy diagram represents the activation complex.
False (B)
Chemical reactions require activation energy to initiate the formation of products.
Chemical reactions require activation energy to initiate the formation of products.
True (A)
The kinetic energy of reacting molecules is precisely the activation energy required for the reaction.
The kinetic energy of reacting molecules is precisely the activation energy required for the reaction.
False (B)
Catalysts function by increasing the activation energy required for a reaction to proceed.
Catalysts function by increasing the activation energy required for a reaction to proceed.
A collision between reactant molecules is always effective in forming products, regardless of orientation or energy.
A collision between reactant molecules is always effective in forming products, regardless of orientation or energy.
Increasing the temperature of a reaction increases the activation energy required for the reaction to proceed.
Increasing the temperature of a reaction increases the activation energy required for the reaction to proceed.
The rate of a chemical reaction is solely dependent on the activation energy; other factors like concentration have no impact.
The rate of a chemical reaction is solely dependent on the activation energy; other factors like concentration have no impact.
If a reaction is exothermic, then the activation energy for the reverse reaction is always lower than the activation energy for the forward reaction.
If a reaction is exothermic, then the activation energy for the reverse reaction is always lower than the activation energy for the forward reaction.
The transition state in a chemical reaction is a stable intermediate that can be easily isolated and characterized.
The transition state in a chemical reaction is a stable intermediate that can be easily isolated and characterized.
For a reaction to occur, all reactant molecules must possess kinetic energy equal to or greater than the activation energy.
For a reaction to occur, all reactant molecules must possess kinetic energy equal to or greater than the activation energy.
Flashcards
Bottom of energy diagram
Bottom of energy diagram
False. The bottom of the energy diagram represents the potential energy of the reactants or products, while the peak represents the activation complex.
Activation Energy Necessity
Activation Energy Necessity
True. Activation energy acts as a barrier that must be overcome for the reaction to proceed.
Kinetic energy vs. Activation energy
Kinetic energy vs. Activation energy
False. Kinetic energy is the energy of motion of the molecules, while activation energy is the minimum energy needed for a reaction.
Catalyst and activation energy
Catalyst and activation energy
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Effective Collision
Effective Collision
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Study Notes
- False. The bottom of the energy diagram represents the reactants or products, not the activation complex (transition state).
- True. Chemical reactions require activation energy to overcome the energy barrier and form products.
- False. Activation energy is the minimum energy required for a reaction to occur, while kinetic energy is the energy of motion possessed by the molecules.
- False. Catalysts decrease the activation energy required for a reaction to proceed.
- False. An effective collision is one where reactants collide with sufficient energy and proper orientation to form products. An ineffective collision does not result in product formation.
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