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### Question 15.39

Posted: Fri Mar 02, 2018 1:05 pm
What equation do we use to determine the time required?

### Re: Question 15.39

Posted: Fri Mar 02, 2018 1:05 pm
Sorry forgot to post the problem, #39:
Determine the time required for each of the following second order reactions to tale place: (A) 2A----> B +C, for the concentration of A to decrease from o.10 mol/L-1 to 0.090mol/L-1, given that k = 0.105L/mol-1/min-1 for the rate law expressed in terms of the loss of a;(B) A------>2B+C, when [A]0 = 0.15 mol/L-1 for the concentration of B to increase to 0.19 mol/L-1, given that k = .0035 L.mol-1*min-1 in the rate law for the loss of A

### Re: Question 15.39

Posted: Fri Mar 02, 2018 1:11 pm
Any of the integrated rate laws relate reaction rate to time.

### Re: Question 15.39  [ENDORSED]

Posted: Fri Mar 02, 2018 3:39 pm
Since it was specified that the reactions are second-order, we can use 1/[A] = kt + 1/[A]0, and just solve for t.

### Re: Question 15.39

Posted: Thu Mar 08, 2018 9:24 pm
Thank you!