Question by kevin n: chem please help?
An experiment that led to the formation of the new field of organic chemistry involved the synthesis of urea, CN2H4O, by the controlled reaction of ammonia and carbon dioxide.
2 NH3(g) + CO2(g) CN2H4O(s) + H2O(l)
What is the theoretical yield of urea when 100. g of ammonia is reacted with 100. g of carbon dioxide?
Answer by mia_in_nz
First step is to find the relative molecular mass (Mr) for each molecule by adding the atomic masses:
Mr(NH3)= 14.01+ 3(1.008)
At this point so i don’t confuse myself later, I times this by 2 since you need two moles to react with 1 mole of CO2
Mr(CO2)= 12.01 + 2(16.00)
Since you’re using the same amount of each compund it’s easy to see at this point that the CO2 will be the limiting reagent, since it’s Mr is greate, therefore the number of moles will be less.
The number of moles (n)= m/Mr
Now the maximum amount of urea able to be produced by this reaction is the smallest number of moles times the Mr of urea
Know better? Leave your own answer in the comments!
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