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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
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