speed of reaction based on activation energy

[FrankieClarke2C]

If a reaction has a higher activation energy, does this mean that the reaction is slower?

[Dimitri Speron 1C]

Yes, generally. This is because the reaction will require a greater buildup of heat in order to reach the energy of its transition state.

[fgalasso1b]

It is because since you need more energy to build up, the longer it takes to acquire the energy for the reaction to take place.

[JT Wechsler 2B]

Typically this is the case. To have a reaction occur, you have to meet a set amount of energy (the activation energy) to have a reaction proceed. Typically the higher the activation energy is, the more energy will be needed to be put into the system.

[mbaker4E]

Yes, because more energy is necessary in order for the reaction to move forward.

[Lorena Zhang 4E]

Yes. To add on that, when adding catalyst, you increase the rate of reaction because the activation energy barrier is lowered so that the reaction can proceed faster.

[Vanadium Wang 4H]

Typically yes because the reaction will require a greater buildup of energy to overcome the activation barrier. Take a look at the Arrhenius Equation:
k = Ae^-(E_A/RT)
A higher activation energy would result in a slower reaction.