Actual Yield Calculator

Calculate actual yield, percent yield, or theoretical yield for chemical reactions. Supports four modes: predict actual yield from efficiency, calculate percent yield from results, find theoretical maximum, or full stoichiometric calculation from limiting reagent.

g

Amount of product actually obtained (g or mol)

g

Maximum possible product from stoichiometry (g or mol)

%

Efficiency percentage (0-100%, >100% indicates error)

g

Mass of limiting reagent (g)

Molar mass of limiting reagent (g/mol)

Coefficient from balanced equation

Molar mass of desired product (g/mol)

Coefficient from balanced equation

Actual = (Percent ÷ 100) × Theoretical Percent = (Actual ÷ Theoretical) × 100% Theoretical = (Actual ÷ Percent) × 100 From Stoichiometry: Moles = Mass ÷ MM; Product = (Moles ÷ CoeffLim) × CoeffProd Loss = Theoretical - Actual Efficiency: 90-100% Excellent, 70-89% Good, 50-69% Moderate, <50% Low
Actual from %: Theoretical=50g, %=85% → Actual = (85÷100)×50 = 42.5g (Loss=7.5g) % Yield: Actual=42.5g, Theoretical=50g → (42.5÷50)×100 = 85% (Good) Theoretical: Actual=30g, %=75% → (30÷75)×100 = 40g Stoichiometry: N₂(14g, MM=28) → NH₃(MM=17), Coeff 1:2 Moles N₂=0.5, Moles NH₃=1.0, Theoretical=17g If Actual=15g: %Yield=(15÷17)×100=88.2% (Good, Loss=2g) Warning: %>100% means impure product or measurement error!

What is actual yield in chemistry?

Actual yield is the amount of product you actually obtain from a chemical reaction when performed in the laboratory. It is measured experimentally after purification. Actual yield is always less than or equal to theoretical yield due to incomplete reactions, side reactions, and product loss during separation and purification steps.

How do I calculate actual yield?

Actual yield is measured, not calculated—you weigh the purified product after the reaction. However, you can predict expected actual yield using: Actual Yield = (Percent Yield ÷ 100) × Theoretical Yield. For example, with 85% yield and 50g theoretical, expect 42.5g actual yield.

Why is actual yield less than theoretical yield?

Several factors reduce actual yield: incomplete conversion (reaction equilibrium), side reactions producing unwanted byproducts, mechanical losses during transfers, evaporation, incomplete purification, and measurement errors. Typical yields: simple reactions 80-95%, complex multi-step syntheses 30-70%.

What does percent yield tell me?

Percent yield = (Actual Yield ÷ Theoretical Yield) × 100%. It measures reaction efficiency. 90-100% is excellent (rare), 70-89% is good, 50-69% is moderate, below 50% needs optimization. Yields over 100% indicate impure product containing water, solvents, or byproducts—always investigate!

How do I improve actual yield?

Optimize reaction conditions (temperature, time, concentration), use excess of cheaper reagents, employ catalysts, use inert atmosphere for air-sensitive reactions, minimize transfers, improve purification techniques, use appropriate drying methods, and consider alternative synthetic routes for problematic steps.

What is the difference between actual, theoretical, and percent yield?

Theoretical yield is the maximum possible product calculated from stoichiometry. Actual yield is what you really get in the lab (measured by weighing). Percent yield relates them: (Actual ÷ Theoretical) × 100%. All three are essential for evaluating reaction success and optimizing synthetic procedures.

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Percent Yield Calculator
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