# chem

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consider the following balance chemical equation:

2NH3(g)+3CuO(s)=N2(g)+3Cu(s)+3H2O(g)

if 18.1grams of ammonia reacts with 90.4 grams of copper(II) oxide, which is the limitting reagent?? what is the theorectical yield of nitrogen gasd? if 8.52 g of N2 are formed, what is the % yield of nitrogn gas??

limitting reagent is NH3 with 2.13 mol N2
theoretical yield nitrogen gas is 59.68g N2
percent yield of nitrogen gas is 14.28%
please i need to know what i'm doing wrong..thank you....

• chem -

No, it isn't correct. From the few numbers you show, I have been able to guess that you have the moles right but you used the wrong conversion to convert to moles N2.
moles NH3 = 18.1/17 = about 1.06
moles N2 = 1.06 x (1 mole N2/2 moles NH3) = 1.06/2 = 0.53 moles N2.

moles CuO = 90.4/79.545 = 1.136
moles N2 formed = 1.136 x (1 mole N2/3 moles CuO) = 1.136*(1/3) = 0.379 moles N2.

I will leave it at that and let you finish but it is important for you to understand that you should have divided by 2 and 3 instead of multiplying by 2 and 3 (at least that's what I think you did).

• chem -

ok..I see what i did wrong...thank u..ur the best!!!

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