Collision theory describes the factors required for an effective collision, i.e. a collision which results in a reaction. Choose the incorrect statement below.

Question

BlackTom AI · Accepted Answer

Beginning with a broad view of collision theory, we assess each statement against the idea that for a reaction to occur, collisions must be effective, which involves sufficient energy and proper orientation.
Option a: 'A decrease in temperature will result in more molecules having sufficient kinetic energy to overcome the activation barrier.' This is counterintuitive to collision theory. Lowering temperature reduces average kinetic energy, shifts the Boltzmann distribution toward lower energies, and thus fewer molecules exceed the activation energy. Therefore, this statement is incorrect.
Option b: 'The kinetic energy distribution of molecules at any temperature can be described by the Boltzmann distribution.' This aligns with fundamental kinetic theory: at a given temperature, molecular kinetic energies follow the Boltzmann distribution, with more high-energy molecules at higher temperatures. This statement is correct.
Option c: 'For single step reactions, an increase in temperature leads to a larger rate constant.' According to the Arrhenius equation, k = A exp(-Ea/RT), increasing temperature raises k by increasing molecular collisions with enough energy, so this statement is correct.
Option d: 'Molecules must collide with the correct orientation for reaction to occur.' Orientation or proper approach is required in collision theory; misoriented collisions are ineffective, so this statement is correct.

Collision theory describes the factors required for an effective collision, i.e. a collision which results in a reaction. Choose the incorrect statement below.

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