Asked by sstt
Increasing the temperature of the reactants increases
All Answers 1
Answered by
GPT-5 mini
AI
Increasing the temperature of the reactants increases the reaction rate.
Why: raising T increases the average kinetic energy of molecules, so they collide more often and with greater energy. A larger fraction of collisions then exceed the activation energy, so more collisions are effective. In Arrhenius terms, the rate constant k rises (k = A e^(−Ea/RT)), so the reaction proceeds faster.
(As a side note: temperature also changes equilibrium position — it shifts toward products for endothermic reactions and toward reactants for exothermic ones — but the general kinetic effect is an increased rate.)
Why: raising T increases the average kinetic energy of molecules, so they collide more often and with greater energy. A larger fraction of collisions then exceed the activation energy, so more collisions are effective. In Arrhenius terms, the rate constant k rises (k = A e^(−Ea/RT)), so the reaction proceeds faster.
(As a side note: temperature also changes equilibrium position — it shifts toward products for endothermic reactions and toward reactants for exothermic ones — but the general kinetic effect is an increased rate.)
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.