Reply 1
To find the mass of methyl 3-nitrobenzoate produced, we need to use the percentage yield and the original mass of methyl benzoate.
First, we need to calculate the theoretical yield of methyl 3-nitrobenzoate by using the molecular weight of both compounds:
Theoretical yield = (1.70 g x 181.0 g/mol) / 136.0 g/mol = 2.26 g
Then, we can use the percentage yield to find the actual yield of methyl 3-nitrobenzoate:
Actual yield = 2.26 g x 65.0% = 1.47 g
Therefore, the answer is C) 1.47 g of methyl 3-nitrobenzoate is produced.
First, we need to calculate the theoretical yield of methyl 3-nitrobenzoate by using the molecular weight of both compounds:
Theoretical yield = (1.70 g x 181.0 g/mol) / 136.0 g/mol = 2.26 g
Then, we can use the percentage yield to find the actual yield of methyl 3-nitrobenzoate:
Actual yield = 2.26 g x 65.0% = 1.47 g
Therefore, the answer is C) 1.47 g of methyl 3-nitrobenzoate is produced.
why
why did you divide 181 by 136
Original post by dulladulla
To find the mass of methyl 3-nitrobenzoate produced, we need to use the percentage yield and the original mass of methyl benzoate.
First, we need to calculate the theoretical yield of methyl 3-nitrobenzoate by using the molecular weight of both compounds:
Theoretical yield = (1.70 g x 181.0 g/mol) / 136.0 g/mol = 2.26 g
Then, we can use the percentage yield to find the actual yield of methyl 3-nitrobenzoate:
Actual yield = 2.26 g x 65.0% = 1.47 g
Therefore, the answer is C) 1.47 g of methyl 3-nitrobenzoate is produced.
First, we need to calculate the theoretical yield of methyl 3-nitrobenzoate by using the molecular weight of both compounds:
Theoretical yield = (1.70 g x 181.0 g/mol) / 136.0 g/mol = 2.26 g
Then, we can use the percentage yield to find the actual yield of methyl 3-nitrobenzoate:
Actual yield = 2.26 g x 65.0% = 1.47 g
Therefore, the answer is C) 1.47 g of methyl 3-nitrobenzoate is produced.
why did you divide 181 by 136
Reply 3
Original post by mblake
why
why did you divide 181 by 136
why did you divide 181 by 136
have the same question here, did you find out why?
the way I would've done it is:
I know % yield = actual/theoretical x 100
They don't give the theoretical in the equation however they do give the Mr and mass of methyl benzoate.
So we can work out the moles of methyl 3-nitrobenzoate by assuming they have a 1:1 and then find the mass of the theoretical yield using the moles.
Moles = mass/mr
0.0125 mols = 1.70/136 (methyl benzoate)
This means methyl 3-nitrobenzoate also has 0.0125 mols.
Then do mass = moles x mr
2.26 = 181 x 0.0125
Then just plug those into the equation:
65.0% = actual / 2.26 x 100
0.65 = actual / 2.26
actual = 1.469
ANS = C (1.47)
(edited 10 months ago)
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