Rate Constants

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

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Ardo 2K
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Joined: Fri Sep 29, 2017 7:05 am

Rate Constants

Why do the rate constants of each molecule being composed or consumed correspond with a different temperature, why aren't they all under standard conditions of 298K?

Srbui Azarapetian 2C
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Joined: Thu Jul 13, 2017 3:00 am
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Re: Rate Constants

The rate constant changes with temperature because the rate of a reaction is dependent on temperature. This has to do with activation energy and the likeliness of a reaction happening because a greater presence of reactants (concentration) or a higher temperature, meaning more kinetic energy, which means molecules are more likely to collide in the right orientation to make the reaction happen. Normally, at higher temperatures, the rate constant increases.

Mitch Mologne 1A
Posts: 74
Joined: Fri Sep 29, 2017 7:04 am

Re: Rate Constants

You could also relate this to our delta g equation last chapter as the higher the temperature is with a positive delta s, the more favorable a reaction is.

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

Re: Rate Constants

I think under different temperature conditions, a reaction can only proceed under a high temperature. The process may be spontaneous but very slow so an increase in temperature will speed up the process. The example given in class was the car to diamond reaction I believe.

Scott Chin_1E
Posts: 55
Joined: Sat Jul 22, 2017 3:00 am

Re: Rate Constants

Another way of explaining this is that at higher temperatures, the particles have much more energy in them and will move more and theoretically "clash" with particles of the other reactant, thus accelerating the speed of the reaction.

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