Gives us a straight line plot.

The slope of the plot we can determine, and that comes out to minus

12516 Kelvin, and we know from the Arrhenius equation that

that's going to be equal to minus the activation energy over R, so now we

have an equality, whereby we can calculate the activation energy.

We know the value of the gas constant R is

8.314 Joules per mole, to degree Kelvin.

So if we multiply the slope by the gas

constant, we will therefore get the

activation energy Ea being equal to

104058 Joules per mole, which is

approximately 104 kilo joules per mole.

So we have now determined the activation energy of the process.

We can also get the exponential factor by

determining the intercept of this plot, and if

we do that, we find that the intercept is equal

to 35.84, which we know is equal to the

natural log of the pre-exponential factor A.

Taking an antilog of that gives you the pre-exponential

factor of 3.686 times 10 to the 15th, the

units here will be per minute because the initial

rates were measured per minute, and we want to get that

into per second, then we are going to have to divide

by 60.

So, we divide that number by 60.

We get 6.143 times 10 to the 13 per second.

We're happy with the units per second, because remember

the pre-exponential factor is essentially related to the collision frequency.

So, this should be units of frequency.

So here we've used the Arrhenius

expression to work out for the decomposition

of N2O5, both the activation energy of

the process and also the pre-exponential factor.

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