Theoretical Yield Calculator

Theoretical Yield Formula:

\[ Theoretical\ Yield = moles\ of\ limiting\ reagent \times stoichiometric\ ratio \times molecular\ weight \]

Theoretical Yield:

Unit Converter ▲

Unit Converter ▼

From:	To:

1. What is Theoretical Yield?

The theoretical yield is the maximum amount of product that can be produced from a given amount of limiting reagent in a chemical reaction, based on stoichiometric calculations.

2. How Does the Calculator Work?

The calculator uses the theoretical yield formula:

\[ Theoretical\ Yield = moles\ of\ limiting\ reagent \times stoichiometric\ ratio \times molecular\ weight \]

Where:

\( moles \) — Amount of limiting reagent in moles
\( stoichiometric\ ratio \) — Mole ratio of product to limiting reagent
\( molecular\ weight \) — Molecular weight of the product in g/mol

Explanation: The calculation determines the ideal maximum yield assuming complete conversion of the limiting reagent to product with no losses.

3. Importance of Theoretical Yield

Details: Theoretical yield is crucial for reaction planning, determining reaction efficiency (actual yield vs theoretical yield), and scaling up chemical processes.

4. Using the Calculator

Tips: Enter the moles of limiting reagent, the stoichiometric ratio of product to limiting reagent, and the molecular weight of the 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 in practice, which is usually lower due to incomplete reactions, side reactions, or losses.

Q2: How do I determine the limiting reagent?
A: The limiting reagent is the reactant that is completely consumed first, limiting the amount of product that can be formed. It's determined by comparing mole ratios.

Q3: What is percentage yield?
A: Percentage yield = (actual yield / theoretical yield) × 100%. It measures the efficiency of a chemical reaction.

Q4: Why is my actual yield lower than theoretical?
A: Common reasons include incomplete reactions, competing side reactions, purification losses, or measurement errors.

Q5: Can theoretical yield be greater than 100%?
A: No, if you get more than theoretical yield, it typically indicates product contamination, measurement errors, or incorrect theoretical calculation.