## Rate Constant K [ENDORSED]

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

Irma Ramos 2I
Posts: 51
Joined: Fri Sep 29, 2017 7:07 am

### Rate Constant K

What exactly does it mean when it says that the rate constant K depends on temperature and activation energy??

Alvin Tran 2E
Posts: 39
Joined: Fri Sep 29, 2017 7:06 am

### Re: Rate Constant K

The value of the rate constant K varies depending on the temperature and activation energy which can be seen through the Arrhenius equation. For example, raising the temperature of the reaction will increase the value of the rate constant K and therefore increase the speed at which the reaction is occurring.

Angel Gomez 1K
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Joined: Fri Sep 29, 2017 7:04 am

### Re: Rate Constant K

You say that k varies depending on activation energy and temperature, but how exactly would we go about calculating the value of k?

Lindsay Kester 2L
Posts: 29
Joined: Thu Jul 27, 2017 3:00 am

### Re: Rate Constant K

Essentially, at different temperatures and activation energies, K changes. You calculate it the same way, using concentrations, but you're going to get a different value at different states. We don't have a way to calculate new K's based on old ones yet, but we might learn one.

Leah Thomas 2E
Posts: 51
Joined: Fri Sep 29, 2017 7:06 am

### Re: Rate Constant K  [ENDORSED]

K constant just describes how fast a reaction can occur. The only way to speed up a reaction is to change the amount of energy input as in raise its temperature or lower the activation energy needed, I. E. Add a catalyst perhaps.