According to the Arrhenius equation k = A e^(-Ea / (RT)), what happens to the rate constant k when the reaction temperature T increases?
Answer and explanation
Correct answer: D. k increases exponentially
- Step 1: In the Arrhenius equation, T appears in the denominator of the negative exponent -Ea/(RT).
- Step 2: As T increases, -Ea/(RT) becomes less negative, so e^(-Ea/(RT)) increases exponentially.
- Step 3: This means a significantly higher proportion of colliding particles possess energy equal to or greater than Ea.
Answer
k increases exponentially.
Why not the others: 'k decreases linearly' is false; temperature increases collision frequency; 'k remains constant' is false because Ea is constant for a given reaction; 'k oscillates based on reactant concentration' confuses rate constants with reaction kinetics.
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