Limiting Reactant

Theoretical Yield

• Concept of theoretical yield: Maximum product yield expected from a reaction under specified conditions.

Limiting Reagents

• Definition: Reactant that is completely consumed in a chemical reaction, determining the amount of product formed.

• Example: Making a sandwich requires specific amounts of ingredients (e.g., 1 slice of cheese, 2 slices of bread).

Calculating Theoretical Yield

• Steps in calculation:

  • Calculate the number of moles of reactants.

  • Use stoichiometric ratios to determine moles of products.

  • Convert moles of product to grams using molar mass.

• Theoretical yield is typically greater than actual yield due to losses in the process.

Example Case Study

• Given: 1.27 grams of copper sulfate and excess zinc metal.

• Calculation yields: 0.392 grams of copper sulfate produced.

• Theoretical moles calculated using stoichiometric ratio 1:1 for copper production.

• Example output: Percentage yield calculated as 77.3%.

• Note: Percentage yield values are generally less than 100% due to practical limitations in reaction processes.