Chemistry Calculation Question
Jeez this is kinda embarrassing.
I have to plan an experiment on producing specifically one gram of aspirin, but I don't even know how to start.
A question I was given was as follows: what mass of ethanoic anhydride would you use to make 1g of aspirin if your predicted yield of aspirin, after purification, is 48%?
I know it has to be to do with calculating moles and stuff but... I'm still useless at all that stuff.
We haven't really been taught this and I'm scared to ask my teacher as I'm consistently handing in late work due to confusion and she doesn't like me anymore.
I have to plan an experiment on producing specifically one gram of aspirin, but I don't even know how to start.
A question I was given was as follows: what mass of ethanoic anhydride would you use to make 1g of aspirin if your predicted yield of aspirin, after purification, is 48%?
I know it has to be to do with calculating moles and stuff but... I'm still useless at all that stuff.
We haven't really been taught this and I'm scared to ask my teacher as I'm consistently handing in late work due to confusion and she doesn't like me anymore.
What have you tried? Any ideas on where to start?
Hi I tried working this out and I hope this helps:
We know that the % yield is 48% and the actual mass of aspirin produced is 1g. % yield = actual mass/ theoretical mass x 100
Therefore 0.48= 1/ theoretical mass
so theoretical mass = 1/0.48
therefore theoretical mass = 2.083g ( this is the mass we will use to find out the moles of aspirin and therefore ethanoic anhydride)
Mols of aspirin = 2.083/(12x9+8+16x4)=0.0115740 mols
ratio = 1:1 therefore mols of ethanoic anhydride = 0.0115740 mols
mass of ethanoic anhydride = 0.0115740 x (12x4 + 6+ 16x3) = 1.1805g
I hope this is right, you might want to look over my working as i'm also a year 12 student and might make some mistakes
We know that the % yield is 48% and the actual mass of aspirin produced is 1g. % yield = actual mass/ theoretical mass x 100
Therefore 0.48= 1/ theoretical mass
so theoretical mass = 1/0.48
therefore theoretical mass = 2.083g ( this is the mass we will use to find out the moles of aspirin and therefore ethanoic anhydride)
Mols of aspirin = 2.083/(12x9+8+16x4)=0.0115740 mols
ratio = 1:1 therefore mols of ethanoic anhydride = 0.0115740 mols
mass of ethanoic anhydride = 0.0115740 x (12x4 + 6+ 16x3) = 1.1805g
I hope this is right, you might want to look over my working as i'm also a year 12 student and might make some mistakes
Original post by smilith
Hi I tried working this out and I hope this helps:
We know that the % yield is 48% and the actual mass of aspirin produced is 1g. % yield = actual mass/ theoretical mass x 100
Therefore 0.48= 1/ theoretical mass
so theoretical mass = 1/0.48
therefore theoretical mass = 2.083g ( this is the mass we will use to find out the moles of aspirin and therefore ethanoic anhydride)
Mols of aspirin = 2.083/(12x9+8+16x4)=0.0115740 mols
ratio = 1:1 therefore mols of ethanoic anhydride = 0.0115740 mols
mass of ethanoic anhydride = 0.0115740 x (12x4 + 6+ 16x3) = 1.1805g
I hope this is right, you might want to look over my working as i'm also a year 12 student and might make some mistakes
We know that the % yield is 48% and the actual mass of aspirin produced is 1g. % yield = actual mass/ theoretical mass x 100
Therefore 0.48= 1/ theoretical mass
so theoretical mass = 1/0.48
therefore theoretical mass = 2.083g ( this is the mass we will use to find out the moles of aspirin and therefore ethanoic anhydride)
Mols of aspirin = 2.083/(12x9+8+16x4)=0.0115740 mols
ratio = 1:1 therefore mols of ethanoic anhydride = 0.0115740 mols
mass of ethanoic anhydride = 0.0115740 x (12x4 + 6+ 16x3) = 1.1805g
I hope this is right, you might want to look over my working as i'm also a year 12 student and might make some mistakes
Thank you very much for your help, this makes a lot of sense - it's a lot less complicated than I thought it might be it seems. I'll have a run through this method myself, thank you very much again.
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