5.5.1 Calculating Percentage Yield

• The actual yield is the amount of product obtained in a chemical reaction
• The actual yield is always greater than the theoretical yield.

  False
• Match the term with its definition and symbol:

  Actual Yield ↔️ The quantity of product obtained in the experiment, $A$

  Theoretical Yield ↔️ The maximum quantity of product calculated from stoichiometry, $T$
• The theoretical yield is the maximum quantity of product that can be calculated from stoichiometry
• Steps to calculate theoretical yield from balanced equations:

  1️⃣ Identify the limiting reactant

  2️⃣ Use the balanced equation to determine molar ratio

  3️⃣ Calculate moles of product

  4️⃣ Convert moles to mass using molar mass
• What is the formula for calculating percentage yield?

  \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100</latex>
• The percentage yield indicates the efficiency of a reaction.
• The actual yield is usually less than or equal to the theoretical yield.
• What is the theoretical yield based on?

  Stoichiometry
• What is the theoretical yield of a chemical reaction based on stoichiometry?

  Maximum amount of product
• Steps to calculate the theoretical yield of a reaction

  1️⃣ Identify the limiting reactant

  2️⃣ Determine the molar ratio

  3️⃣ Calculate the moles of product

  4️⃣ Convert moles to mass
• In the reaction 2H_{2} + O_{2} \rightarrow 2H_{2}O</latex>, $H_{2}$ is the limiting reactant if 4g of it reacts with excess $O_{2}$
• If 2 moles of $H_{2}$ react, then 2 moles of $H_{2}O$ are produced based on the 1:1 ratio
• What is the theoretical yield of $H_{2}O$ in grams if 2 moles are produced?


  36g
• Match the term with its definition:

  Theoretical yield ↔️ Maximum product based on stoichiometry

  Limiting reactant ↔️ Reactant consumed first

  Molar ratio ↔️ Ratio of moles between reactants and products
• The percentage yield is the ratio of actual yield to theoretical yield, expressed as a percentage
• What is the formula for calculating percentage yield?

  $\frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100$
• Match the term with its definition and units:

  Actual Yield ↔️ Amount of product obtained in the lab (g or mol)

  Theoretical Yield ↔️ Maximum product based on stoichiometry (g or mol)

  Percentage Yield ↔️ Ratio of actual yield to theoretical yield (%)
• If the theoretical yield is 50g and the actual yield is 40g, the percentage yield is 80%
• The percentage yield indicates the efficiency of a reaction.
• What is the formula for calculating percentage yield?

  \frac{\text{Actual Yield}}{\text{Theoretical Yield}} \times 100</latex>
• If the theoretical yield is 60g and the actual yield is 45g, the percentage yield is 75%