Stoichiometry Calculator
Analyze chemical equations and determine reactant and product ratios
Stoichiometry Calculator
Analyze chemical equations and determine reactant and product ratios
Enter Chemical Equation
Format: Use + to separate compounds and = or → for reaction arrow. Include coefficients if known.
Balanced Chemical Equation
Stoichiometric Ratios
Reactant Ratios
Product Ratios
About Stoichiometry
Stoichiometry is the branch of chemistry that deals with the quantitative relationships between reactants and products in chemical reactions. It allows chemists to predict the amounts of substances that will be consumed and produced in a reaction.
The stoichiometric ratio, represented by the coefficients in a balanced chemical equation, shows the relative number of moles of each substance involved in the reaction.
Types of Stoichiometry
Mole-to-Mole Stoichiometry
Converts moles of one substance to moles of another using the stoichiometric ratio from the balanced equation.
Mass-to-Mass Stoichiometry
Converts grams of one substance to grams of another by using molar masses and stoichiometric ratios.
Mole-to-Mass Stoichiometry
Converts moles of one substance to the mass of another using the stoichiometric ratio and molar mass.
Mass-to-Mole Stoichiometry
Converts grams of one substance to moles of another using molar mass and the stoichiometric ratio.
Stoichiometric Coefficients
In balanced chemical reactions, the numbers written in front of each compound are called stoichiometric coefficients. These coefficients indicate the relative number of moles of each substance.
Example: 4Fe + 3O2 → 2Fe2O3
- 4 is the coefficient for Fe (iron)
- 3 is the coefficient for O2 (oxygen gas)
- 2 is the coefficient for Fe2O3 (iron(III) oxide)
This means: 4 moles of Fe react with 3 moles of O2 to produce 2 moles of Fe2O3.
Example Problem
Problem:
Given the balanced equation: 2H2 + O2 → 2H2O, how many grams of water are produced when 4.0 grams of hydrogen reacts with excess oxygen?
Solution:
Step 1: Calculate molar masses
- H2 = 2(1.008) = 2.016 g/mol
- H2O = 2(1.008) + 16.00 = 18.016 g/mol
Step 2: Convert grams to moles
Moles of H2 = 4.0 g ÷ 2.016 g/mol = 1.98 mol
Step 3: Use stoichiometric ratio
From equation: 2 mol H2 → 2 mol H2O
Moles of H2O = 1.98 mol × (2 mol H2O / 2 mol H2) = 1.98 mol
Step 4: Convert moles to grams
Grams of H2O = 1.98 mol × 18.016 g/mol ≈ 35.7 g
Answer: Approximately 35.7 grams of water are produced
Common Atomic Masses (g/mol)
Important Notes
- • Stoichiometry calculations require balanced chemical equations
- • The stoichiometric ratio comes directly from the coefficients in the balanced equation
- • Molar mass is the mass of one mole of a substance, expressed in g/mol
- • In limiting reagent problems, stoichiometry helps identify which reactant runs out first
- • Always check your units and ensure they cancel properly in calculations
Frequently Asked Questions about Stoichiometry
What is stoichiometry and why is it important?
Stoichiometry is the study of the quantitative relationships between reactants and products in chemical reactions. It allows chemists to predict how much of each substance will be consumed and produced, making it essential for chemical manufacturing, laboratory work, and understanding reaction outcomes.
What are stoichiometric coefficients?
Stoichiometric coefficients are the numbers written in front of chemical formulas in a balanced equation. They represent the mole ratio of reactants to products. For example, in 2H₂ + O₂ → 2H₂O, the coefficients are 2, 1, and 2, meaning 2 moles of hydrogen react with 1 mole of oxygen to produce 2 moles of water.
Why must chemical equations be balanced?
Chemical equations must be balanced to satisfy the Law of Conservation of Mass, which states that matter cannot be created or destroyed in a chemical reaction. This means the number of each type of atom must be the same on both the reactant and product sides of the equation.
What is molar mass and how is it calculated?
Molar mass is the mass of one mole of a substance, expressed in grams per mole (g/mol). It's calculated by adding the atomic masses of all atoms in a compound. For example, H₂O has a molar mass of (2 × 1.008) + 16.00 = 18.016 g/mol. You can look up atomic masses on the periodic table.
How do I use stoichiometry to solve chemistry problems?
Stoichiometry problems typically follow these steps: (1) Start with a known quantity (grams, moles, liters), (2) Convert to moles if needed using molar mass, (3) Use stoichiometric ratios from the balanced equation to convert to moles of desired substance, (4) Convert to desired units (grams, liters, etc.) using molar mass or gas laws.
What is the difference between theoretical yield and actual yield?
Theoretical yield is the amount of product that would be produced if the reaction went to completion and no side reactions occurred, calculated using stoichiometry. Actual yield is what you really get in the lab, which is usually less due to incomplete reactions, side reactions, and losses during transfer. Percent yield = (Actual/Theoretical) × 100%.
What is a limiting reagent?
A limiting reagent is the reactant that runs out first in a chemical reaction, determining the maximum amount of product that can be formed. To find it, calculate how much product each reactant can produce and the one that produces the least is the limiting reagent. Stoichiometry is essential for identifying limiting reagents.
Can I use this calculator to balance chemical equations?
No, this calculator assumes the equation is already balanced. If your equation is unbalanced, you'll need to balance it first using the coefficient method, inspection method, or algebraic methods. Many online equation balancers can help if you're unsure.
Pro Tips
- • Always verify that your chemical equation is balanced before performing stoichiometric calculations.
- • Mole-to-mole ratios come directly from stoichiometric coefficients. Use them to convert between different substances.
- • When converting grams to grams, you need three pieces: starting mass → moles → moles of product → product mass.
- • For gas problems at STP, remember that 1 mole of gas occupies 22.4 liters. For other conditions, use the ideal gas law (PV = nRT).
- • In limiting reagent problems, calculate product amount for each reactant separately. The smallest amount is your actual yield.
- • Pay attention to units throughout your calculation. Dimensional analysis helps ensure your units cancel correctly.
- • Remember that stoichiometry only works with balanced equations. If percentages don't add up, your equation might not be balanced.
- • Use scientific notation for very large or very small numbers to avoid calculation errors.
Update Logs
View the latest updates and features