7D.1

Arrhenius Equation:

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Jason Wu 1E
Posts: 101
Joined: Thu Jul 25, 2019 12:15 am

7D.1

Postby Jason Wu 1E » Tue Mar 10, 2020 10:26 pm

The rate constant of the first-order reaction 2 N2O(g) -> 2 N2(g) + O2(g) is 0.76 s^-1 at 1000. K and 0.87 s^-1 at 1030. K. Calculate the activation energy of the reaction.

How do we approach this question? are we supposed to substitute for k and T into Arrhenius's Equation to create a system of equations to solve for A and Ea? How do we do this calculation?

Katherine Wu 1H
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Joined: Fri Aug 30, 2019 12:15 am
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Re: 7D.1

Postby Katherine Wu 1H » Tue Mar 10, 2020 10:34 pm

we use ln(k prime/k) = (Ea/R)(1/T-1/T prime) = (Ea/R)((T prime-T)/T(T prime))
ln (k prime/k)=ln(0.87 s^-1/0.76 s^-1)
=(Ea/8.31x10^-3 kJ/K.mol)((1030K-1000K)/(1030Kx1000K))
Ea=((8.31x10^-3kJ/K.mol)(1000K)(1030K)/(1030K-1000K))ln(0.87 s^-1/0.76 s^-1)
=39 kJ/mol

Shannon Asay 1C
Posts: 102
Joined: Fri Aug 09, 2019 12:16 am

Re: 7D.1

Postby Shannon Asay 1C » Tue Mar 10, 2020 10:36 pm

I believe you could use the equation ln(k2/k1)=-Ea/R*(1/T2-1/T1). Just plug in all your variables and solve for Ea.

Jessa Maheras 4F
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Joined: Fri Aug 02, 2019 12:16 am

Re: 7D.1

Postby Jessa Maheras 4F » Wed Mar 11, 2020 6:28 pm

Shannon Asay 1C wrote:I believe you could use the equation ln(k2/k1)=-Ea/R*(1/T2-1/T1). Just plug in all your variables and solve for Ea.


Yes, I agree! All you do is rearrange the equation and plug in values.

Aman Sankineni 2L
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Joined: Fri Aug 30, 2019 12:17 am

Re: 7D.1

Postby Aman Sankineni 2L » Wed Mar 11, 2020 7:02 pm

The equation ln(k2/k1)=-Ea/R*(1/T2-1/T1) should be able to be used.


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