The Arrhenius equation shows that the rate constant increases when
- A. the activation energy increases
- B. the temperature falls
- C. the activation energy decreases or the temperature rises
- D. the concentration of reactants rises
Explanation
The equation contains an exponential term in which activation energy appears with a negative sign and temperature in the denominator, so lowering the barrier or raising the temperature both increase k, and the dependence is exponential rather than linear. This is why a catalyst and a temperature rise produce such large changes in rate. Concentration does not appear in the equation at all.