### Question 15.39

Posted:

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

Created by Dr. Laurence Lavelle

https://lavelle.chem.ucla.edu/forum/

https://lavelle.chem.ucla.edu/forum/viewtopic.php?f=145&t=28756

Page **1** of **1**

Posted: **Fri Mar 02, 2018 1:05 pm**

What equation do we use to determine the time required?

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

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

Posted: **Fri Mar 02, 2018 1:11 pm**

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

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.

Posted: **Thu Mar 08, 2018 9:24 pm**

Thank you!