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 has a high activation energy and a low orientation factor. Predict the rate of this reaction and explain your reasoning.
Describe how the concentration of reactants affects the rate of reaction according to collision theory.
Describe the role of the orientation factor in determining the rate of a chemical reaction.
Describe the term 'effective collision' in the context of collision theory.
A reaction has a high activation energy and a low orientation factor. Predict the rate of this reaction and explain your reasoning.
Calculate the number of effective collisions per second if the total number of collisions is 1.0 × 109 and only 1 in 106 collisions is effective.
If a reaction has a low activation energy and a high orientation factor, what can you say about its rate?
If the activation energy of a reaction is 50 kJ/mol and the average kinetic energy of molecules is 40 kJ/mol, will the reaction proceed rapidly? Explain.
The collision theory is most successful in explaining the kinetics of which type of reactions? (1) Complex reactions (2) Elementary reactions (3) Photochemical reactions (4) Nuclear reactions
The collision theory was first proposed by which scientist(s)? (1) Arrhenius (2) Boltzmann and Maxwell (3) Lewis and Clark (4) Rutherford
The orientation factor (p) in collision theory is usually: (1) Greater than 1 (2) Equal to 1 (3) Less than 1 (4) Zero
The rate constant (k) in the Arrhenius equation is related to which aspect of collision theory? (1) Frequency of collisions (2) Activation energy (3) Orientation factor (4) All of the above
Fill in the blank: For a collision to be effective, the colliding molecules must have energy equal to or greater than the __________ energy and must be properly oriented.
Fill in the blank: The __________ equation mathematically relates the rate constant to temperature and activation energy.
Fill in the blank: The __________ factor in the Arrhenius equation accounts for the orientation of molecules during collisions.
Fill in the blank: The __________ theory explains the effect of molecular orientation and energy on the rate of chemical reactions.
True or False: According to collision theory, every collision between reactant molecules leads to the formation of products.
True or False: According to collision theory, increasing the temperature increases both the frequency and the effectiveness of collisions.
True or False: Increasing the surface area of a solid reactant increases the rate of reaction by increasing the number of possible collisions.
True or False: The activation energy is the energy difference between the reactants and the products.
