If 10g of NO react with 20g of O2, what is the maximum amount of NO2 that can be produced? How do I know exactly which is limiting and which is excess, is there a calculation that shows this?

Answer 1

In order to find the limiting and/ or excess reactant, you have to first convert grams to moles, then once you have that you did the #s by the smallest mole #. Once you have that, you compare that to the coefficients of the balanced equation.

Answer 2

This was my answer, but it was wrong:

2NO + O2 ----> 2NO2

Molar Mass NO2 = 46g/mol
Molar mass NO = 30g/mol
Molar Mass O2 = 32g/mol

0.333 mols NO x 46g NO2/1mol NO = 15.3g NO2

mols NO = 10g NO/30g/1mol NO = 0.333 mols NO
mols O2 = 20g O2/32g O2/1mol O2 = 0.625 mols O2

Where did I mess up?? And how do I figure out what is limiting reactant and what is excess?

Answer 3

Am i solving this correctly, according to my answer/posts above??

Answer 4

Ok, so you just do .333/.333 =1 (NO)
and .625/.333= 1.87 (O2)

So, then you go back to your equation, and you see how 1 < 2(# of moles of NO in the equation), that means it is the limiting reactant

Then you do the same thing with 1.87, and 1.87> 1( # of mole of O2), so that tells you it is the excess reactant. Make sense?

Answer 5

I guess so, thanks "K"

Answer 6

Tmofey, you didn't do anything wrong in your chemistry. I think the problem is math. I see 20g and 30g as having 2 significant figures so you can't report more than 2 in your answer. If you are keying this into a database, as I suspect, those things are notoriously unforgiving for the number of s.f. So your answer is 15.3 g NO2, you are allowed only 2 s.f., round the answer to 15 g NO2 produced. I'll bet the database accepts that answer.

Answer 7

I will do that, thanks for your help once again DrBob222.