Chemical Equation Balancer
Use + between compounds and -> or → between reactants and products
About Chemical Equation Balancing
Law of Conservation of Mass: Matter cannot be created or destroyed in a chemical reaction. The number of atoms of each element must be the same on both sides.
Coefficients: Numbers placed before formulas to balance the equation. They multiply all atoms in that compound.
Example: 2H₂ + O₂ → 2H₂O means 4 hydrogen atoms and 2 oxygen atoms on each side.
Understanding Chemical Equation Balancing
Balancing chemical equations is a fundamental skill in chemistry. A balanced equation shows that the number of atoms of each element is conserved during a chemical reaction.
Law of Conservation of Mass
The Law of Conservation of Mass states that matter cannot be created or destroyed in a chemical reaction. This means the total mass of reactants must equal the total mass of products. When we balance equations, we ensure that atoms are conserved.
Steps to Balance Equations
- Write the unbalanced equation with correct formulas
- Count the atoms of each element on both sides
- Add coefficients to balance atoms (start with most complex molecule)
- Balance hydrogen and oxygen last
- Check that all atoms are balanced
- Reduce coefficients to smallest whole numbers
Example: Combustion of Methane
Unbalanced: CH₄ + O₂ → CO₂ + H₂O
- Reactants: 1 C, 4 H, 2 O
- Products: 1 C, 2 H, 3 O
Balanced: CH₄ + 2O₂ → CO₂ + 2H₂O
- Reactants: 1 C, 4 H, 4 O
- Products: 1 C, 4 H, 4 O
Types of Chemical Reactions
- Synthesis: A + B → AB (e.g., 2H₂ + O₂ → 2H₂O)
- Decomposition: AB → A + B (e.g., 2H₂O → 2H₂ + O₂)
- Single Replacement: A + BC → AC + B
- Double Replacement: AB + CD → AD + CB
- Combustion: Fuel + O₂ → CO₂ + H₂O
Tips for Balancing
- Never change subscripts in formulas (only coefficients)
- Balance metals first, then non-metals
- Balance polyatomic ions as a group if they appear unchanged
- Use fractional coefficients temporarily, then multiply to get whole numbers