-(a) A certain first-order reaction has a rate constant of 2.75 × 10–2 s–1 at 20 °C. What is the value of k at 60 °C if Ea = 75.5 kJ/mol?
(b) Another first-order reaction also has a rate constant of 2.75 × 10–2 s–1 at 20 °C. What is the value of k at 60 °C if Ea = 125 kJ/mol?
(c) What assumptions do you need to make in order to calculate answers for parts (a) and (b)?
(a) ln(k2/k1) = Ea/R[1/T1 - 1/T2]
with,
k1 = 2.75 x 10^-2 s-1
k2 = rate constant at 6- oC = ?
T1 = 20 + 273 = 293 K
T2 = 60 + 273 = 333 K
Ea = 75.5 kJ/mol
R = gas constant
we get,
ln(k2/2.75 x 10^-2) = 75500/8.314[1/293 - 1/333]
k2 at 60 oC = 1.14 s-1
(b) Again using the same equation and taking values from above,
ln(k2/2.75 x 10^-2) = 125000/8.314[1/293 - 1/333]
k2 at 60 oC = 13.07 s-1
(c) We have used Arrhenius equation in both (a) and (b) case. The ssumption is to be made that the rate constant would be higher at higher temperature.
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