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?
Calculate the fraction of molecules with energy equal to or greater than the activation energy if Ea = 50 kJ/mol, R = 8.314 J/mol·K, and T = 298 K. Use the expression e−Ea/RT.
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.
Describe the effect of increasing the concentration of one reactant on the rate of reaction according to collision theory.
Describe the role of activation energy in determining whether a collision is effective or not.
Explain how increasing the surface area of a solid reactant affects the rate of reaction according to collision theory.
Explain the term 'collision frequency' and its significance in chemical reactions.
Explain why increasing the temperature increases the rate of reaction according to collision theory.
Explain why not all collisions between reactant molecules lead to a chemical reaction.
Explain why the collision theory is less accurate for reactions involving complex molecules.
In a reaction between gases A and B, what will happen to the rate of reaction if the pressure is doubled?
State the main postulates of the collision theory of chemical reactions.
The collision theory equation for the rate constant (k) is k = Z × P × e−Ea/RT. What does Z represent?
What is meant by the term 'effective collision' in collision theory?
What is the significance of the steric factor in collision theory?
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.
Consider the following scenario: In a reaction between molecules X and Y, it is observed that even though the collision frequency is high, the reaction rate is low. Based on collision theory, suggest two possible reasons for this observation.
For a bimolecular reaction, the rate constant k is given by k = Z × P × e−Ea/RT. If the steric factor P is much less than 1, what does this indicate about the orientation requirements for the reaction?
