Sapling #11

[Rylee Mangan 1K]

Can anyone help me start this problem or tell me which lecture to find the material?

Dinitrogen pentoxide, N2O5, decomposes by first‑order kinetics with a rate constant of 3.7×10−5 s−1 at 298 K.
What is the half‑life, in hours, of N2O5 at 298 K?

Thanks!

[Jonathan Haimowitz 3B]

The question states that this decomposition is first-order, so use the first-order half life equation:
Note that it asks for the half-life in hours, and the result of this equation will be in seconds.

[RDove_3G]

Hi, all the information on half-life equations is given in today's lecture, lecture 23. The rate constant you are given is k and it is a first-order reaction so you want to use the equation for a first-order half-life which is ln2/k. Be careful of units.

[Daniela Santana 2L]

Hi! In order to solve for the half life of something you use the equation t1/2 = ln2/k. ln2 approximately equals .693 so solve for .693/3.7x10^-5. The value you get from this will be in seconds so be sure to convert this value to hours by applying 60 as many times needed. I hope this helps!!