Let's consider the following example:

A chemist is attempting to synthesize a compound called Compound X through a simple reaction. The balanced chemical equation for the reaction is:

2 A + 3 B → Compound X

To perform this reaction, the chemist starts with 10 grams of A and 15 grams of B.

1. Theoretical Yield Calculation:
The theoretical yield is the maximum amount of product that can be obtained based on stoichiometry. In this case, the stoichiometry of the reaction tells us that 2 moles of A react with 3 moles of B to produce 1 mole of Compound X.

a) Convert the given masses of A and B into moles:
Molar mass of A = 20 g/mol
Molar mass of B = 40 g/mol

Moles of A = 10 g / 20 g/mol = 0.5 mol
Moles of B = 15 g / 40 g/mol = 0.375 mol

b) Determine the limiting reactant:
Based on the balanced equation, it is clear that 2 moles of A react with 3 moles of B. Therefore, B is the limiting reactant since there are only 0.375 moles of B available, which is less than the necessary 0.667 moles (0.375 mol * 3/2).

c) Calculate the theoretical yield:
Since B is the limiting reactant, we use its moles to determine the product yield.
Theoretical yield of Compound X = 0.375 mol * (1 mol of Compound X / 3 mol of B) = 0.125 mol

2. Actual Yield Calculation:
After performing the reaction, the chemist obtained 0.100 moles (or 10 grams) of Compound X.

3. Percent Yield Calculation:
Percent yield is a measure of the efficiency of a reaction and is calculated by dividing the actual yield by the theoretical yield and multiplying by 100.

Percent Yield = Actual Yield / Theoretical Yield * 100
Percent Yield = 0.100 mol / 0.125 mol * 100 = 80%

Therefore, the chemist achieved an 80% percent yield in this reaction.

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