At 100 degrees C , a certain substance undergoes second-order decomposition with a half-life of 26 minutes.

Question

If the initial concentration of the substance is 3.9×10−2M , what is the value of the rate constant at 100degrees C?

So I put in (1560seconds) 1/2 = 1/ k (3.9×10−2M) and end up getting 2.5x10^-5

What am I doing wrong? :[

Answer 1

1560=1/k*3.9E-2

k=1/(1560*3.9E-2)=1/60.84=1.64E-2

I don't think you calculated with Ao in the denominator.

Answer 2

You are most correct, I did not.
Thank you so much.