With the increase of 10°C temperature, the rate of reaction doubles. This increase in rate of reaction is due to:
Correct answer: D. Increase in number of effective collision
- A. Decrease in activation energy of reaction
- B. Decrease in the number of collision between molecules of reactants
- C. Increase in activation energy of molecules of reactants
- D. Increase in number of effective collision
Explanation
When the temperature increases by 10°C, the rate of reaction doubles because of an increase in effective collisions. The higher temperature provides more kinetic energy to the particles, causing them to move faster and collide more frequently. This leads to a greater chance of successful collisions and an increased rate of reaction. The activation energy remains the same, but the increased temperature helps overcome this energy barrier more easily.
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About Reaction Kinetics
Reaction kinetics relates reaction rate to concentration, temperature, surface area and catalysts. Questions cover rate laws, reaction order, rate constants, activation energy and the activated complex, including how a catalyst lowers the activation energy without changing the overall energy change or equilibrium position.
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