Consider three reactions with different values of E_a and ΔE:

Reaction 1. E_a = 20 kJ>mol; ΔE = -60 kJ/mol

Reaction 2. E_a = 10 kJ>mol; ΔE = -20 kJ/mol

Reaction 3. E_a = 40 kJ>mol; ΔE = +15 kJ/mol

(b) Assuming that all three reactions are carried out at the same temperature and that all three have the same frequency factor A, which reaction is the fastest and which is the slowest?

Video transcript

Hello everyone today. We have the following problem. The following reactions have the same frequency factor and are performed at the same temperature. So we have reaction A. B and C determine which reaction is the slowest and which is the fastest. So before we do that, let's make note that the activation energy or sub A. Is what determines which is the slowest or the fastest reaction. And in which way? Well we can say that the higher the activation energy, the slower the reaction. Make note that the activation energy is the energy required to get a reaction started. So if you need a lot of energy to sort of reaction of course it is going to be considered slower than if you needed Just a little bit of energy, the reaction would proceed faster. So of the above reactions that we have here reaction or reactions B. And A. Have the highest and lowest activation energy respectively. If we look at the activation energies here, we can make a note of that. With that being said, reaction B has a higher reaction reaction B has a higher activation energy and is therefore the slowest and reaction A. Has the lowest activation energy, activation energy and is therefore the fastest and the answer choice that best some of this up is answer choice B. Reaction B is the slowest because it has the highest activation energy reaction A is the fastest because it has the lowest activation energy. And with that we've answered the question overall. I hope that this helped and until next time