A first order reaction has a rate constant of 0.816 at 25 oC. Given that the activation energy is 22.7 kJ/mol, calculate the rate constant at 34 oC. (enter answer to 3 decimal places)

1.067

Explanation:

Using the Arrhenius equation relates rate constants to the temperature is:

ln(k2/k1) = −Ea/R * [1/T2−1/T1]

where,

Ea = activation energy in kJ/mol ,

R = universal gas constant, and

T = temperature in K .

T1 = 25 + 273.15

= 298.15 K

T2 = 34 + 273.15

= 307.15 K

k1 = 0.816

Therefore,

k2/k1 = exp(-22.7/0.008314472) * [1/307.15 −1/298.15 ])

= 0.816 * 1.308

k2 = 1.067.

m=9

step-by-step explanation: