in reaction S + O2 -> SO2, determine percent yield if 4 grams of S produced 64 gram of SO2
mols S = 4/atomic mass S.
Convert mols S to mols SO2.
Convert mols SO2 to g SO2 by g = mols x molar mass. This is the theoretical yield.Then
%yield = (actual yield/theor yield)*100 = ?
thank you
To determine the percent yield in a chemical reaction, you need to compare the actual yield (the amount of product obtained) with the theoretical yield (the maximum amount of product that can be obtained according to stoichiometry). The percent yield can be calculated using the formula:
Percent Yield = (Actual Yield / Theoretical Yield) * 100
First, let's find the theoretical yield. In the balanced chemical equation:
S + O2 -> SO2
The stoichiometric ratio between S and SO2 is 1:1. This means that for every mole of S reacted, one mole of SO2 is produced. To convert grams to moles, you need to know the molar mass of sulfur (S) and sulfur dioxide (SO2).
The molar mass of S = 32 g/mol.
The molar mass of SO2 = (1 × atomic mass of S) + (2 × atomic mass of O) = (1 × 32) + (2 × 16) = 64 g/mol.
To find the moles of S:
Moles of S = Mass of S / Molar mass of S
Moles of S = 4 g / 32 g/mol = 0.125 mol
Since the stoichiometric ratio between S and SO2 is 1:1, the moles of SO2 produced will also be 0.125 mol.
Now, let's calculate the theoretical yield of SO2:
Theoretical Yield = Moles of SO2 * Molar mass of SO2
Theoretical Yield = 0.125 mol * 64 g/mol = 8 g
The theoretical yield is 8 grams of SO2.
Now, we can calculate the percent yield:
Percent Yield = (Actual Yield / Theoretical Yield) * 100
Percent Yield = (64 g / 8 g) * 100
Percent Yield = 800%
The percent yield is 800% in this case. However, it is important to note that this value is greater than 100%, which indicates a mistake in measurement or calculation. Percent yield cannot exceed 100% in a real experimental scenario.