Asked by Sar
At 100 degrees C , a certain substance undergoes second-order decomposition with a half-life of 26 minutes.
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? :[
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? :[
Answers
Answered by
bobpursley
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.
k=1/(1560*3.9E-2)=1/60.84=1.64E-2
I don't think you calculated with Ao in the denominator.
Answered by
Sar
You are most correct, I did not.
Thank you so much.
Thank you so much.
There are no AI answers yet. The ability to request AI answers is coming soon!
Submit Your Answer
We prioritize human answers over AI answers.
If you are human, and you can answer this question, please submit your answer.