Theoretical Yield Calculator

Theoretical Yield Formula:

\[ \text{Yield} = \text{Moles of Reactant} \times \text{Stoichiometric Ratio} \times \text{Molecular Weight of Product} \]

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 in a chemical reaction based on the amount of limiting reactant. It represents the ideal outcome if the reaction proceeds perfectly with no losses.

2. How Does the Calculator Work?

The calculator uses the theoretical yield formula:

\[ \text{Yield} = \text{Moles of Reactant} \times \text{Stoichiometric Ratio} \times \text{Molecular Weight of Product} \]

Where:

Moles of Reactant — Amount of limiting reactant in moles
Stoichiometric Ratio — Mole ratio of product to reactant from balanced equation
Molecular Weight of Product — Molar mass of the product in g/mol

Explanation: The calculation converts moles of reactant to moles of product using the stoichiometric ratio, then converts to grams using the product's molecular weight.

3. Importance of Theoretical Yield

Details: Theoretical yield is crucial for predicting reaction outcomes, calculating percent yield, and determining reaction efficiency. It helps chemists plan experiments and assess their success.

4. Using the Calculator

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

5. Frequently Asked Questions (FAQ)

Q1: How is theoretical yield different from actual yield?
A: Theoretical yield is the calculated maximum possible, while actual yield is what you obtain in practice, usually lower due to incomplete reactions or losses.

Q2: What is percent yield?
A: Percent yield = (Actual Yield / Theoretical Yield) × 100%. It measures reaction efficiency.

Q3: How do I find the stoichiometric ratio?
A: From the balanced chemical equation - it's the coefficient of the product divided by the coefficient of the reactant.

Q4: What if I have multiple reactants?
A: You must first identify the limiting reactant - the one that would produce the least product based on its moles and stoichiometry.

Q5: Why is my actual yield lower than theoretical?
A: Common reasons include incomplete reactions, side reactions, product loss during transfer/purification, or measurement errors.