00:01
This question is in a reference to chemical kinetics, and it wants to know which of the following statements is false.
00:07
The first one says changing the temperature does not change the activation energy for a reaction.
00:14
This is true according to the arranius equation, k is equal to a multiplied by e to the negative ea over rt.
00:30
The activation energy is a constant.
00:35
If we change the temperature, the constant stays the same, but although ea doesn't change, the rate constant does change with a change in temperature.
00:47
So that one is true.
00:49
The next one says at higher temperature, a higher percent of reactants, have enough energy to reach the transition state.
00:57
This is also true because at higher temperatures, we have more collisions that have enough energy to overcome the activation energy, and overcoming the activation energy is the same thing as reaching the transition state.
01:19
If we had an energy diagram, this would be the transition state, and this would be the activation energy.
01:29
So having enough energy to reach the transition state means enough energy to overcome activation...