Asked by Bobz

What would the units of the rate constant k be in a second order equation if rate was measured in mol/(L x s)and all concentrations in mol/L

a)L/(mol x s)
b)L2/(mol2 x s)
c)L3/(mol3 x s)
d)mol2/(L2 x s)

I think it's b) or a)
Answered by DrBob222
<b>I tried to make this look pretty by using superscripts but it is painstaking to do it AND if I forgot to make one tiny tiny error it screws up; so if it looks funny, I'll try redoing it but using the conventional caret for superscripts.</b>
Why are you guessing? Work it out.
rate = k(A)<sup>2</sup>
(mol/L*s) = k((mol/L)<sup>2</sup>
(mol/L*s) = k*(mol<sup>2</sup>/L<sup>2</sup>
To clear the fraction, multiply both sides by (L<sup>2</sup>/mol<sup>2</sup> to obtain
(mol/L*s)*(L<sup>2</sup>/mol<sup>2</sup> = k(mol<sup>2</sup>/L<sup>2</sup>)*(L<sup>2</sup>/mol<sup>2</sup>)
All of that on the right side cancels, except for k and on the left you have remaining, L/mol*s if I didn't make an algebra error. Here is a site that gives you the answer.
http://www.scribd.com/doc/11579759/Examvillecom-Units-of-Reaction-Rate-Constant
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