Asked by Maya
A second-order reaction has a rate constant of 1.65 M–1 s–1. If the initial reactant concentration is 1.0 M, calculate the time (in seconds) required for the reaction to become 90% complete.
i got 0.06734 seconds but that's incorrect i have no idea what i am doing wrong! HELP!!!!
i got 0.06734 seconds but that's incorrect i have no idea what i am doing wrong! HELP!!!!
Answers
Answered by
DrBob222
The equation is
[1/(A)] - [1/(Ao)] = kt
Ao = 1
A = 0.1 if it is to be 90% complete.
k is given.
Solve for t.
I plugged in your number for t and apparently you substituted 0.9 for (A) but if it's 90% complete, that means A is 0.1. Try that, see if it doesn't work.
[1/(A)] - [1/(Ao)] = kt
Ao = 1
A = 0.1 if it is to be 90% complete.
k is given.
Solve for t.
I plugged in your number for t and apparently you substituted 0.9 for (A) but if it's 90% complete, that means A is 0.1. Try that, see if it doesn't work.
Answered by
Anonymous
The way DrBob222 did is correct.
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.