Theoretical Yield Calculator

Limiting Reagent

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Molecular weight:

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Stoichiometry (Optional):

Desired Product

Mole(s):

Molecular weight:

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Theoretical Yield Calculator

Use this theoretical yield calculator to find the maximum amount of product that can be formed from a given chemical reaction. It also calculates the limiting reagent and the stoichiometry of the product between the moles of reactants and the product formed.

What Is Theoretical Yield?

Theoretical yield is the maximum quantity of the product that can be produced from a given amount of reactants in a chemical reaction. The maximum possible product formed under 100% efficiency.

Theoretical Yield Formula:

By using the given formula, we can find the theoretical yield from the moles of the limiting reagent:

m_product = n_{limiting reactant} × C_Product C_{limiting reactant} × M_product

✅ Simple form:

m_product = n_lim × C_product C_lim × M_product

Where:

m_product = Mass of the product
n_lim = Number of moles of the limiting reagent
M_mol,product = Molar mass of the product (g/mol)
C_lim = Stoichiometric coefficient of the product in the balanced equation

To calculate the moles of the limiting reagent:

n_{limiting reactant} = n m

Note: Keep in mind that all stoichiometric calculations, including finding the limiting reagent and using the theoretical yield formula, require you to have a balanced chemical equation.

How To Calculate Theoretical Yield?

For theoretical yield calculation, follow these steps:

Balance the Chemical Equation
Recognize The Limiting Reactant
Determine The Moles of Limiting Reagent
Use The Theoretical Yield Equation

Theoretical Yield Example:

Consider the reaction of aluminum with hydrochloric acid to produce aluminum chloride and hydrogen gas: 27 g of aluminum reacts with 60 g of hydrochloric acid (HCl). Determine the theoretical yield of hydrogen gas (H₂).

Solution:

Step 1: Write the Balanced Chemical Equation

2 Al + 6 HCl → 2 AlCl₃ + 3 H₂

Step 2: Identify the Given Data

Mass of Al = 27 g
Mass of HCl = 60 g
Molar masses:
- Al = 27 g/mol
- HCl = 36.5 g/mol
- H₂ = 2 g/mol

Step 3: Calculate Moles of Each Reactant

Moles of Al = 27 ÷ 27 = 1 mol

Moles of HCl = 60 ÷ 36.5 ≈ 1.64 mol

Step 4: Determine the Limiting Reactant

From the equation, 2 mol Al reacts with 6 mol HCl.
Required HCl for 1 mol Al = (6/2) × 1 = 3 mol HCl
We only have 1.64 mol HCl, which is less than required.
Therefore, HCl is the limiting reagent.

Step 5: Calculate Moles of H₂ Produced

From the balanced equation: 6 HCl → 3 H₂

Moles of H₂ = (3/6) × 1.64 = 0.82 mol H₂

Step 6: Convert Moles of H₂ to Mass

Mass of H₂ = 0.82 × 2 = 1.64 g

Final Answer:

The theoretical yield of H₂ is 1.64 g.

Summary:

Limiting reagent: HCl (1.64 moles)
Theoretical yield of H₂ = 1.64 g

You can easily simplify these calculations by using our chemistry theoretical yield calculator and make an informed decision to optimize the chemical process.

How To Use The Theoretical Yield Calculator?

Step 1: Input Limiting Reagent

Mass of The Limiting Reagent: Input the mass of the limiting reagent
Molecular Weight: Enter the molecular weight of the limiting reagent
Stoichiometry: If available then you should provide the stoichiometry ratio

Step 2: Input Desired Product

Moles of Product: Enter the moles of the expected product in the designated field
Molecular Weight of the Product: Provide the molecular weight of the product

Step 3: Calculate

Click on the “Calculate” button and the calculator will provide the theoretical yield in grams, along with some additional information

Why Is It Important To Calculate Theoretical Yield?

Calculating theoretical yield is important for various reasons, including:

Reaction Optimization: Helps to recognize the area for improvement by comparing the actual and theoretical yield
Resource Management: Minimize the waste by providing the maximum product yield
Estimating the Cost: By calculating the theoretical yield, industries can easily predict the final product cost
Maintaining Product Quality: Determines the amount of reactant required to form the quality product
Understanding The Mechanisms of Reactions: Finding theoretical yield provides insight into chemical processes and side reaction

How Theoretical Yield Depends on Reaction Conditions

However, it can be obtained under perfect conditions, where no product is lost in the process.

Ideal Conditions for Theoretical Yield:

No impurities mixed in the reactants
No production of unexpected products that can reduce the yield
There is no loss of product because of any measurement, processing, and handling of reactants or products

Limiting Reagent:

In a chemical reaction, the limiting reagent is a reactant that is completely used up first. It helps to determine how much product can be formed. Meanwhile, it limits" the amount of product that is formed in a chemical reaction.

Stoichiometry:

Stoichiometry is the study of relationships between reactants and products in chemical reactions. It finds the mole ratios of reactants and products, helping you understand how much quantity of a substance is needed to react with another substance.

The numbers in front of each ingredient in a chemical reaction are the reactant's stoichiometry. If no number is found, then the stoichiometry is said to be 1. Keep in mind that stoichiometry is needed to reflect the ratios of molecules that come together to form a product.

Research Sources:

From ChemLibreTexts – Theoretical Yield, covering excess and limiting reagents.

From OneClass – How to calculate theoretical yield of aspirin.

Theoretical Yield Calculator

Theoretical Yield Calculator

What Is Theoretical Yield?

Theoretical Yield Formula:

How To Calculate Theoretical Yield?

Theoretical Yield Example:

How To Use The Theoretical Yield Calculator?

Step 1: Input Limiting Reagent

Step 2: Input Desired Product

Step 3: Calculate

Why Is It Important To Calculate Theoretical Yield?

How Theoretical Yield Depends on Reaction Conditions

Ideal Conditions for Theoretical Yield:

Limiting Reagent:

Stoichiometry:

People Also Ask:

What is The Effect of Concentration on Yield?

What is the Difference Between Theoretical Yield and Actual Yield?

Research Sources: