he rate constant of a chemical reaction increased from 0.100 s ? 1 to 3.00 s ? 1

Question

he rate constant of a chemical reaction increased from 0.100 s?1 to 3.00s?1 upon raising the temperature from 25.0 ?C to 35.0?C . Part A Calculate the value of (1T2?1T1) where T1 is the initial temperature and T2 is the final temperature.
he rate constant of a chemical reaction increased from 0.100 s?1 to 3.00s?1 upon raising the temperature from 25.0 ?C to 35.0?C . he rate constant of a chemical reaction increased from 0.100 s?1 to 3.00s?1 upon raising the temperature from 25.0 ?C to 35.0?C . Part A Calculate the value of (1T2?1T1) where T1 is the initial temperature and T2 is the final temperature.
Part A Calculate the value of (1T2?1T1) where T1 is the initial temperature and T2 is the final temperature.

Explanation / Answer

Set up two Arrhenius equations with these two sets of variables:

k1 = Ae^(-E_a/(RT1))
k2 = Ae^(-E_a/(RT2))

These can be combined by dividing one by the other:

k1/k2 = (Ae^(-E_a/(RT1)))/(Ae^(-E_a/(RT2)))

The A factor cancels out, then after rearrangement and some math, one should get a form by which E_A can be calculated (all the other variables are knowns).

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