what would be the percent yield if 2.2 grams of aspirin is formed?
%yield = (actual yield/theoretical yield)*100 = ?
You give neither the theoretical yield nor a way to calculate it.
To calculate the percent yield of a chemical reaction, you need to know the theoretical yield and the actual yield. The theoretical yield is the maximum amount of product that can be obtained based on the balanced chemical equation, while the actual yield is the amount of product obtained experimentally.
In this case, you have been given the actual yield of 2.2 grams of aspirin. To determine the theoretical yield, you would need additional information such as the balanced chemical equation and the molar mass of aspirin.
Assuming the balanced chemical equation for the reaction is:
2 C9H8O4 + H2O → 2 C7H6O3 + C4H6O3
And the molar mass of aspirin (C9H8O4) is approximately 180.16 g/mol, you can calculate the theoretical yield as follows:
(2.2 g aspirin) × (1 mol/180.16 g) = 0.0122 mol aspirin
To find the percent yield, you need to divide the actual yield by the theoretical yield and multiply by 100:
Percent Yield = (Actual Yield / Theoretical Yield) × 100
Percent Yield = (2.2 g / (0.0122 mol × 180.16 g/mol)) × 100
Without the additional information mentioned above, it is not possible to calculate the percent yield accurately.
To determine the percent yield, you need to know the theoretical yield and the actual yield of aspirin. The theoretical yield is the maximum amount of product that can be obtained from a given amount of reactants, based on stoichiometry. The actual yield is the amount of product obtained in reality through the experiment.
To calculate the percent yield, you need to know the balanced chemical equation for the reaction that produces aspirin. Let's assume the balanced equation is:
2C7H6O3 + C4H6O3 -> 2C9H8O4 + H2O
In this equation, 2 moles of C7H6O3 react with 1 mole of C4H6O3 to produce 2 moles of C9H8O4 (aspirin) and 1 mole of H2O.
Next, you need to determine the molar mass of aspirin (C9H8O4). Carbon has a molar mass of approximately 12.01 g/mol. Hydrogen has a molar mass of about 1.01 g/mol, and oxygen has a molar mass of around 16.00 g/mol.
Calculating the molar mass of aspirin:
C9H8O4 = 9(12.01 g/mol) + 8(1.01 g/mol) + 4(16.00 g/mol)
= 180.16 g/mol
Now, you can calculate the theoretical yield of aspirin. Convert the given mass of aspirin (2.2 grams) to moles:
moles = mass / molar mass
moles = 2.2 g / 180.16 g/mol
moles ≈ 0.0122 mol
From the balanced equation, you can see that 2 moles of C7H6O3 react to produce 2 moles of C9H8O4 (aspirin). Therefore, the theoretical yield of aspirin from 0.0122 moles of C7H6O3 would be:
theoretical yield = 2 (moles of aspirin)
theoretical yield = 2 * 0.0122 mol
theoretical yield ≈ 0.0244 mol
Finally, you can calculate the percent yield using the formula:
percent yield = (actual yield / theoretical yield) * 100
Since you have not provided the actual yield in this case, you cannot calculate the percent yield without that information. The percent yield is a measure of how efficient a reaction is, so it requires both the theoretical and actual yield values.