[tonedeafminstrel]

My friends and I have been trying to find out how this works "On assumption that catalyst lowers the activation energy twice, it is true that k₂/k₁=2"....We don't understand why, could someone please explain?

[Dan]

"On assumption that catalyst lowers the activation energy twice,

What does that mean?

[Borek]

"On assumption that catalyst lowers the activation energy twice,

What does that mean?

That reaction gets 7.389 times faster?

tonedeafminstrel: http://en.wikipedia.org/wiki/Arrhenius_equation

[tonedeafminstrel]

Thanks! My friends and I managed to figure it out this morning. Turns out the answer was written wrong.

[Dan]

"On assumption that catalyst lowers the activation energy twice,

What does that mean?

That reaction gets 7.389 times faster?

Yes, I took it to mean E_a2/E_a1 = 2

In which case, k₂/k₁ = 2 is wrong

[charco]

you need to use the Arrhenius equation

k = Ae^-Ea/RT

Look at the effect of doubling Ea on k (the rate constant) while keeping the other variables constant (i.e. the temperature amd the actual reaction)