(adsbygoogle = window.adsbygoogle || []).push({}); 1. The problem statement, all variables and given/known data

A certain reaction, with an activation energe of 64.5 kJ/mole, is run at 25.0'C (degree Celsius) and its rate is measured. How many times faster would this reaction be if it were run at 50.0'C (degree Celsius)?

2. Relevant equations

I think: (Arrhenius equation)

ln(k1/k2) = Ea/R (1/T2 - 1/T1)

R = 8.314 J/mole*K

3. The attempt at a solution

I don't know where to start. Only Ea = 64.5 kJ/mole, 1 temperature = 25.0'C and R (8.314 J/mole*K) are given. I don't know where to get the other numbers to plug in the equation.

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# Homework Help: Chemistry: Activation Energy (Arrhenius equation)

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