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:
k1 = rate constant at T1
k2 = rate constant at T2
Ea = activation energy (in J/mol)
R = gas constant (8.314 J/mol•K)
T1 and T2 = temperature (in K).
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
E. none of these
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Arrhenius Equation concept. You can view video lessons to learn Arrhenius Equation. Or if you need more Arrhenius Equation practice, you can also practice Arrhenius Equation practice problems.
What is the difficulty of this problem?
Our tutors rated the difficulty ofIncreasing the reaction temperature from 25°C to 30°C raises...as medium difficulty.