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.
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.
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.
Explain how increasing the temperature affects the rate of a chemical reaction according to collision theory.
Explain the significance of the activation energy in a chemical reaction.
Explain why increasing the pressure of a gas increases the rate of reaction according to collision theory.
Explain why not all collisions between reactant molecules result in a chemical reaction.
Explain why the collision theory is less accurate for reactions involving complex molecules.
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.
In a reaction between A and B, if the activation energy is high, what can you infer about the rate of reaction?
State the two main conditions required for a collision to result in a chemical reaction according to collision theory.
A certain reaction between gases X and Y is observed to proceed much faster when the reactants are heated from 300 K to 320 K. Using collision theory, explain in detail why this increase in temperature leads to a significant increase in the reaction rate, even though the total number of collisions does not double.
A reaction between two molecules, A and B, has a very high collision frequency but a very low rate constant. Using collision theory, provide a detailed explanation for this observation.
Consider a reaction where the rate constant k is given by the Arrhenius equation: k = A e−Ea/RT. If the activation energy (Ea) is 75 kJ mol−1 and the pre-exponential factor (A) is 2.0 × 1012 s−1, calculate the rate constant at 350 K. (R = 8.314 J mol−1 K−1)
Explain why, according to collision theory, reactions between ions in aqueous solution are generally much faster than reactions between covalent molecules.
In a hypothetical reaction, the orientation factor (p) is 0.01 and the collision frequency (Z) is 2.0 × 1010 s−1. If the fraction of collisions with sufficient energy (f) is 1.0 × 10−4, calculate the number of effective collisions per second.
