Collision Theory of Chemical Reactions
Chemistry ⇒ Chemical Kinetics and Equilibrium
Collision Theory of Chemical Reactions starts at 11 and continues till grade 12.
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A reaction between two gases is found to proceed faster at higher temperatures. Explain this observation using collision theory.
A reaction has a high activation energy. According to collision theory, what can you say about its rate at room temperature?
Describe how pressure affects the rate of reaction for gaseous reactants according to collision theory.
Describe the effect of a catalyst on the activation energy of a reaction according to collision theory.
A reaction between two gases is found to proceed faster at higher temperatures. Explain this observation using collision theory.
A reaction has a high activation energy. According to collision theory, what can you say about its rate at room temperature?
In a reaction between gases A and B, what will happen to the rate of reaction if the pressure is doubled?
A certain reaction between two gases has a very low rate constant at 300 K but a much higher rate constant at 500 K. Using collision theory, explain why the rate constant increases so significantly with temperature, considering both the energy distribution of molecules and the activation energy.
The rate constant (k) in the collision theory equation is affected by which of the following?
(1) Temperature
(2) Pressure
(3) Both (1) and (2)
(4) Neither (1) nor (2)
The rate of a chemical reaction depends on which of the following?
(1) Frequency of collisions
(2) Energy of collisions
(3) Orientation of molecules
(4) All of the above
Which factor does NOT affect the rate of effective collisions in a chemical reaction?
(1) Temperature
(2) Catalyst
(3) Color of reactants
(4) Concentration of reactants
Which of the following best describes the effect of a catalyst on a chemical reaction?
(1) Increases activation energy
(2) Decreases activation energy
(3) Increases the energy of reactants
(4) Decreases the energy of products
Fill in the blank: The __________ energy is the energy difference between the reactants and the activated complex.
Fill in the blank: The __________ theory considers both the energy and orientation of colliding molecules in explaining reaction rates.
Fill in the blank: The collision theory explains the effect of __________ on the rate of reaction by considering the kinetic energy of molecules.
Fill in the blank: The fraction of collisions that have energy equal to or greater than the activation energy is called the __________ factor.
True or False: According to collision theory, increasing the concentration of reactants increases the rate of reaction.
True or False: According to collision theory, the rate of reaction is directly proportional to the number of effective collisions per unit time.
True or False: The collision frequency is the number of collisions per unit time per unit volume.
True or False: The collision theory assumes that molecules are rigid spheres.
