Chemistry- two point Arrhenius Equation (miscalculation?)

[Flip]

Chemistry- two point Arrhenius Equation (miscalculation??)

Homework Statement

At 25 degrees celsius, the first-order rate constant for a reaction is 2.0 x 10^3 s^-1. The activation energy is 15.0 kJ/mol. what is the value of the rate constant at 75 degrees celsius.

T1= 298.15 K
T2= 348.15 K
K1= 2.0 x 10^3 s^-1
Ea= 15.0 kJ/mol
K2= ??

Homework Equations

K2=K1(e^[(Ea/R)(1/T1-1/T2)])

The Attempt at a Solution

K2= 2.0 x 10^3 s^-1(e^[(15.0 kJ/mol / 8.3145 J/molK)(10^3 J / 1 kJ)(0.0036 K - 0.0029 K)])

I can't remember if the solution is supposed to be 4.8 x 10^3 s^-1. This is taken from my notes that I have on my course guide. I am basically trying to replicate the entire process, but I keep coming up with over sized answers that are to the 9th power or something... -.-

 

[link2110]

lol i can't understand your work...try using the super and subscripts and latex...then maybe people can read what you're trying to say

 

[Blueshift5]

The solution for the rate constant at 75 degrees celsius (K2) should be 4.8 x 10^3 s^-1. However, your calculation may have been incorrect due to a miscalculation in the Arrhenius equation. It is important to double-check your calculations and ensure that all units are consistent. Additionally, it may be helpful to use scientific notation to avoid large numbers and potential errors. If you are still getting significantly different values, it may be worth consulting with your instructor or a peer for further clarification and assistance.