Could someone please help me with a chemistry problem?

Question

This is the question:
A certain first order reaction has a rate constant of .0275 at 20 degrees C. What is the value of k at 60 degrees C if the activation energy is 75.5 kj/mol.

So, K1 is .0275, k2 is unknown, T1 is 293 in kelvin, T2 is 333 k, and the activation energy is 75.5. I used this formula to solve the problem -
ln(k1/k2) = Ea/R (1/T2 - 1/t1)
So, (.0275/k2) = e to the ((75.5/8.31)((1/333)-(1/293)). then i got .0275/.9962, which is the wrong answer. The right answer is 1.1. Could someone please explain what I am doing wrong?

I did use R=8.31. Please try and show me work if you answer.

Answer 1

Try using R as 8.314 J/(mole)(K) which is equivalent to what you used but with different units. You should have examples in your text where they work these problems, so you can see this.

Good luck.