Homework Help: Chemistry, Arrhenius law

Posted by Donna on Wednesday, May 28, 2008 at 12:23am.

The rate constant of a first order reaction is 4.60x10^-4/s at 350 degrees Celsius. If the activation energy is 104 kJ/mol, calculate the temp. at which its rate constant is 8.80 x 10^-4/s.

So I think that I can use this version of the equation:

ln (k1/k2) = Ea/R * (T1-T2/T1*T2)

Because I am looking for T2.
But now how do I go about solving for T2 when it's in two different places like that?

Chemistry, Arrhenius law - DrBob222, Wednesday, May 28, 2008 at 12:59am
How about trying this? k1, k2, Ea, R are known, so lets just use them as constants and call T1 something like 300.
ln K = k(300-X/300X)
?? = k(300-X/300X)
300X*??= k(300-X)
300X*?? = 300k - 300X
300*??*X + 300X = 300*k
Which is similar to
400X+300X = 400
700X = 400
X = 400/700
I know I have not made sense with the values but it shows you how to solve the problem.

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