Problem: Increasing the reaction temperature from 25°C to 30°C raises the reaction rate 7.5- fold. What is the rate constant for the at 27.5 °C? Activation energy is 3.03x105 J/molA. 6.2 x 10-4B. 1.3 x 102C. 4.6 x 10-7D. 11.3E. none of these

FREE Expert Solution

We’re being asked to determine the rate constant at 25°C of the reaction when k = 8.54 x 10-4 s -1 at 45°C with a EA = 90.8 kJ


This means we need to use the two-point form of the Arrhenius Equation:


lnk2k1 = -EaR1T2-1T1


where:

k1 = rate constant at T1 

k2 = rate constant at T

Ea = activation energy (in J/mol) 

R = gas constant (8.314 J/mol•K) 

T1 and T2 = temperature (in K).

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Problem Details

Increasing the reaction temperature from 25°C to 30°C raises the reaction rate 7.5- fold. What is the rate constant for the at 27.5 °C? Activation energy is 3.03x105 J/mol

A. 6.2 x 10-4

B. 1.3 x 102

C. 4.6 x 10-7

D. 11.3

E. none of these

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