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Balancing Chemical Equations

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Balancing Chemical Equations

Use coefficients to balance chemical equations. The number of atoms of each element must be the same on both sides. Change coefficients only—never change a formula’s subscripts.

Understand the symbols

1.What does the coefficient in front of a chemical formula tell you?
  • How many whole molecules or formula units are represented
  • How many different elements are in the substance
  • Which element the substance will become
  • How many atoms are in the nucleus
2.Which equation has equal numbers of every type of atom on both sides?
  • 2 H₂ + O₂ → 2 H₂O
  • H₂ + O₂ → H₂O
  • H₂ + 2 O₂ → 2 H₂O
  • 2 H₂ + 2 O₂ → H₂O
3.Select all statements that correctly describe balancing equations.
  • Atoms are rearranged during a reaction, not created or destroyed.
  • Changing a subscript is an acceptable way to balance an equation.
  • A coefficient applies to every atom in the formula that follows it.
  • A balanced equation has the same number of each type of atom on both sides.

Balance the equations

Write the smallest whole-number coefficients. A coefficient of 1 may be left unwritten.

4.Balance: H₂ + O₂ → H₂O
5.Balance: N₂ + H₂ → NH₃
6.Balance: Fe + O₂ → Fe₂O₃
7.Balance the combustion equation: C₃H₈ + O₂ → CO₂ + H₂O
8.Balance: Al + O₂ → Al₂O₃
9.Explain how a coefficient differs from a subscript in a chemical formula.
10.Challenge: Balance the equation, keeping the groups of atoms together where possible: Ca(OH)₂ + HCl → CaCl₂ + H₂O

2 printable pages

  • Balancing Chemical Equations, page 1 of 2: Understand the symbols, Balance the equations

    Page 1

  • Balancing Chemical Equations, page 2 of 2: 5. Balance: N₂ + H₂ → NH₃

    Page 2

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