Theoretical Yield Calculator From Equation

Theoretical Yield Formula:

\[ \text{Theoretical Yield} = \text{moles limiting} \times \text{stoich} \times \text{MW} \]

Theoretical Yield:

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1. What is Theoretical Yield?

The theoretical yield is the maximum amount of product that can be produced in a chemical reaction based on the amount of limiting reagent. It assumes perfect efficiency and complete conversion of reactants to products.

2. How Does the Calculator Work?

The calculator uses the theoretical yield formula:

\[ \text{Theoretical Yield} = \text{moles limiting} \times \text{stoich} \times \text{MW} \]

Where:

\( \text{moles limiting} \) — Moles of the limiting reagent (mol)
\( \text{stoich} \) — Stoichiometric ratio of product to limiting reagent
\( \text{MW} \) — Molecular weight of the product (g/mol)

Explanation: The calculation accounts for the mole ratio between reactants and products in the balanced chemical equation and converts this to mass using the product's molecular weight.

3. Importance of Theoretical Yield

Details: Theoretical yield is crucial for determining reaction efficiency (actual yield/theoretical yield × 100%), planning chemical syntheses, and calculating reagent requirements.

4. Using the Calculator

Tips: Enter moles of limiting reagent, stoichiometric ratio from balanced equation, and molecular weight of product. All values must be positive numbers.

5. Frequently Asked Questions (FAQ)

Q1: What is the difference between theoretical and actual yield?
A: Theoretical yield is the calculated maximum possible yield, while actual yield is what you obtain experimentally, which is usually lower due to incomplete reactions, side reactions, or losses.

Q2: How do I find the limiting reagent?
A: Compare mole ratios of all reactants to the stoichiometric ratios in the balanced equation. The reactant with the smallest ratio (moles available/stoichiometric coefficient) is limiting.

Q3: What if my reaction has multiple products?
A: Calculate theoretical yield separately for each product using the appropriate stoichiometric ratio for that product.

Q4: Why is my actual yield higher than theoretical?
A: This could indicate product contamination, incomplete drying, or measurement errors. Theoretical yield represents the absolute maximum possible.

Q5: How accurate is this calculation?
A: The calculation is mathematically precise, but assumes 100% reaction efficiency and perfect stoichiometry. Real-world yields are typically lower.