Question

The rate constant of a reaction(K) is 0.0047 at 298k and the activation energy is 33.6 Kj/mol. What is K at 348K?

T1- 298
T2- 348
K1- 0.0047
K2-?
Ea- 33.6 Kj/mol

I keep getting 1.01 S^-1 but the textbook says its 0.033 s^-1

Answer 1

Ln*K2 =0.0092 is as far as I can get.

Answer 2

are you using the two-point form Arrhenius equation?

Answer 3

Ln (k2/k1) = -Ea/r((1/t2)-(1/t1))
This is the equation that I'm using

Answer 4

\(\large ln\dfrac{k_2}{k_1}=-\dfrac{E_a}{R}(\dfrac{1}{T_2}-\dfrac{1}{T_1})\)

raise both sides to e

\(\large \dfrac{k_2}{k_1}=e^{(\small-\dfrac{E_a}{R}(\dfrac{1}{T_2}-\dfrac{1}{T_1}))}\)

move \(k_1\) over
\(\large k_2=k_1e^{(\small-\dfrac{E_a}{R}(\dfrac{1}{T_2}-\dfrac{1}{T_1}))}\)

Answer 5

Ah! I get it now! I was multiplying K1 to the other side and then taking the anti-log of that and that's how I got 1.01. Thanks for the help!

Answer 6

yeah, logarithms are funny to work with, good stuff though! no problem