## Question 15.39 [ENDORSED]

$aR \to bP, Rate = -\frac{1}{a} \frac{d[R]}{dt} = \frac{1}{b}\frac{d[P]}{dt}$

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Joined: Fri Sep 29, 2017 7:05 am

### Question 15.39

What equation do we use to determine the time required?

Posts: 50
Joined: Fri Sep 29, 2017 7:05 am

### Re: Question 15.39

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

Emily Mei 1B
Posts: 50
Joined: Fri Sep 29, 2017 7:04 am

### Re: Question 15.39

Any of the integrated rate laws relate reaction rate to time.

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Joined: Fri Sep 29, 2017 7:04 am

### Re: Question 15.39  [ENDORSED]

Since it was specified that the reactions are second-order, we can use 1/[A] = kt + 1/[A]0, and just solve for t.