Actual Yield Calculator
Calculate actual yield, percent yield, or theoretical yield for chemical reactions
Calculate Chemical Yields
Maximum possible yield based on stoichiometry
Reaction efficiency (typically 50-95%)
Yield Formulas
Actual Yield: Ya = (Yp / 100) × Yt
Percent Yield: Yp = (Ya / Yt) × 100
Theoretical Yield: Yt = Ya / (Yp / 100)
Where: Ya = Actual yield, Yp = Percent yield, Yt = Theoretical yield
Example Calculation
Precipitation Reaction
Reaction: AgNO₃ + NaCl → AgCl + NaNO₃
Theoretical yield: 4.0 g AgCl (calculated from stoichiometry)
Percent yield: 85% (experimental efficiency)
Step-by-Step Solution
1. Apply actual yield formula: Ya = (Yp / 100) × Yt
2. Substitute values: Ya = (85% / 100) × 4.0 g
3. Calculate: Ya = 0.85 × 4.0 g = 3.4 g
4. Interpretation: You obtained 3.4 g of AgCl from your precipitation reaction
Result: 3.4 g actual yield (85% efficiency)
Common Reaction Examples
Simple Precipitation
Theoretical: 10 g, Actual: 8.5 g
85% yield
Organic Synthesis
Theoretical: 5.2 g, Actual: 3.7 g
72% yield
Crystallization
Theoretical: 15.8 g, Actual: 14.5 g
92% yield
Acid-Base Reaction
Theoretical: 7.6 g, Actual: 5.9 g
78% yield
Oxidation Reaction
Theoretical: 12.3 g, Actual: 8 g
65% yield
Combustion Analysis
Theoretical: 4.4 g, Actual: 3.9 g
89% yield
Yield Efficiency Guide
Yield Tips
Theoretical yield assumes 100% conversion
Actual yield is usually lower than theoretical
Percent yield indicates reaction efficiency
Yields over 100% suggest impurities
Always use consistent units
Understanding Chemical Yields
Types of Yield
Theoretical Yield
Maximum amount of product possible from stoichiometric calculations, assuming 100% conversion.
Actual Yield
Amount of product actually obtained from the experiment, typically less than theoretical.
Percent Yield
Ratio of actual to theoretical yield, expressed as percentage. Indicates reaction efficiency.
Factors Affecting Yield
Yield Losses
- • Incomplete reactions (equilibrium)
- • Side reactions and by-products
- • Product loss during purification
- • Measurement and transfer errors
Yield Gains
- • Incomplete drying (solvent present)
- • Impurities in final product
- • Measurement errors
- • Atmospheric moisture absorption
Stoichiometry and Yield Calculations
Calculating Theoretical Yield
1. Balance the chemical equation
2. Identify the limiting reagent
3. Use mole ratios to find product moles
4. Convert moles to mass using molar mass
Example: Combustion of Methane
Reaction: CH₄ + 2O₂ → CO₂ + 2H₂O
Given: 14 g CH₄, excess O₂
Step 1: 14 g CH₄ ÷ 16.04 g/mol = 0.873 mol CH₄
Step 2: 0.873 mol CH₄ × 1 mol CO₂/mol CH₄ = 0.873 mol CO₂
Step 3: 0.873 mol × 44.01 g/mol = 38.4 g CO₂ (theoretical)
Step 4: If actual = 26.9 g, then percent yield = 70%