Question

question 11 (1 point)
the rate of a chemical reaction is doubled for every 10 °c rise in temperature. this is because of a
decrease in activation energy
increase in activation energy
increase in number of ineffective collisions
increase in the number of effective collisions
increase in enthalpy

Explanation:

1. Activation Energy: Activation energy is the minimum energy for a reaction. Temperature rise doesn't change activation energy (so options about its change are wrong).
2. Collisions: Higher temperature increases molecular kinetic energy. More molecules have energy ≥ activation energy, so effective collisions (those causing reaction) increase. Ineffective collisions would decrease as effective ones rise.
3. Enthalpy: Enthalpy (ΔH) is about reaction heat, not reaction rate from temperature (so enthalpy increase is irrelevant).

Only "increase in the number of effective collisions" explains the rate doubling with temperature (more effective collisions → faster rate).

Answer:

D. increase in the number of effective collisions (Note: Assuming the options are labeled A - E, with this as the correct one. If original labels differ, adjust, but the content is the correct reasoning.)