Arrhenius Equation:

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Lucia H 2L
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Joined: Mon Nov 14, 2016 3:00 am
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Postby Lucia H 2L » Wed Mar 14, 2018 8:00 pm

The rate constant of the reaction O(g) + N2(g) --> NO(g) + N(g), which takes place in the stratosphere, is
9.7 x 10^10 L mol-1 s-1 at 800 deg C. The activation energy of the reaction is 315 kJ mol-1. Determine the rate constant at 700 deg C.

What is the first step here? Do you need to solve for lnA in the Arrhenius equation?

Angela G 2K
Posts: 30
Joined: Fri Sep 29, 2017 7:06 am

Re: 15.109

Postby Angela G 2K » Wed Mar 14, 2018 10:24 pm

You don't need lnA here. You have the rate constant at 800 deg C and the question asks for the rate constant for the same reaction at 700 deg C, so you have these two equations:

At Temp 1 = 800 C = 1073 K:
At Temp 2 = 700 C = 973 K:

Combine them and you get
Simplify to get

Plug in the values and solve for k2.

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