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Chemistry- two point Arrhenius Equation (miscalculation??)
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= ??
K2=K1(e^[(Ea/R)(1/T1-1/T2)])
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... -.-
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... -.-