Answer:
Limiting reagent: NH3
moles of Urea = 0.45 moles
Explanation:
To do this, all we need to do is to see the balanced reaction which is:
2NH3 + CO2 ----------> (NH2)2CO + H20
Now, the leading numbers in the molecules mean in other words, the theorical moles that are needed to get this reaction.
So according to the reaction, 2 moles of NH3 reacts with 1 mol of CO2. Now, let's see how many moles do we actually have with the initial data:
moles of NH3 = 15.33/17.03 = 0.9 moles
moles of CO2 = 0.6 moles
Now that we have the moles, let's see which is the limiting reagent:
If:
2 NH3 -------> 1 CO2 then:
0.9 -----------> X
Solving for X:
X = 0.9 * 1 / 2 = 0.45 theorical moles of CO2
And we have 0.6 moles of CO2, which mean that we have in excess the CO2, therefore, the limiting reagent is the NH3. Let's prove it:
2NH3 -------> 1 CO2
X ----------> 0.6 moles
X = 0.6 * 2 / 1 = 1.2 theorical moles of NH3
And we have 0.9 moles of NH3. So this is a proof that NH3 is the limiting reagent as we state before.
As the NH3 is the limiting reagent, this means that in the reaction all the moles of NH3 will be consumed in the reaction and then, it will produce moles of urea.
Remanent moles of CO2 = 0.6 - 0.45 = 0.15 moles of CO2
moles of NH3 at the end of reaction: 0
moles of urea = 0.45 moles
