- Identify reactants: \(C_4H_{10}O\) and \(O_2\), and products: \(CO_2\) and \(H_2O\).
- Balance carbon by adding a coefficient of 4 to \(CO_2\).
- Balance hydrogen by adding a coefficient of 5 to \(H_2O\).
- Balance oxygen by adding a coefficient of 6 to \(O_2\), yielding the balanced equation \(\boxed{C_4H_{10}O(l) + 6O_2(g) \rightarrow 4CO_2(g) + 5H_2O(l)}\).
Explanation
- Identifying Reactants and Products
The reaction involves the complete combustion of n-butanol, which has the chemical formula \(C_4H_{10}O\). Complete combustion occurs when an organic compound reacts with oxygen gas (\(O_2\)) to produce carbon dioxide (\(CO_2\)) and water (\(H_2O\)). The reaction can be represented by the following unbalanced skeleton equation:
\[C_4H_{10}O(l) + O_2(g) \rightarrow CO_2(g) + H_2O(l)\]
- Balancing the Chemical Equation
To balance the equation, we must ensure that the number of atoms of each element is the same on both sides of the arrow.
- Carbon (C): There are 4 carbon atoms in one molecule of \(C_4H_{10}O\). To balance this, we place a coefficient of 4 in front of \(CO_2\):
\[C_4H_{10}O + O_2 \rightarrow 4CO_2 + H_2O\]
- Hydrogen (H): There are 10 hydrogen atoms in one molecule of \(C_4H_{10}O\). To balance this, we place a coefficient of 5 in front of \(H_2O\) (since \(5 \times 2 = 10\)):
\[C_4H_{10}O + O_2 \rightarrow 4CO_2 + 5H_2O\]
- Oxygen (O): Now, we count the total number of oxygen atoms on the right side: \(4 \times 2\) (from \(CO_2\)) + \(5 \times 1\) (from \(H_2O\)) = 13 oxygen atoms. On the left side, we already have 1 atom in the \(C_4H_{10}O\) molecule. Therefore, we need \(13 - 1 = 12\) more oxygen atoms, which must come from the \(O_2\) molecule. Since each \(O_2\) molecule provides 2 atoms, we need 6 molecules of \(O_2\) (\(6 \times 2 = 12\)).
\[C_4H_{10}O + 6O_2 \rightarrow 4CO_2 + 5H_2O\]
- Final Balanced Equation
The final balanced chemical equation for the combustion of n-butanol is:
\[C_4H_{10}O(l) + 6O_2(g) \rightarrow 4CO_2(g) + 5H_2O(l)\]
All elements are balanced: 4 carbons, 10 hydrogens, and 13 oxygens on both sides.
Examples
Combustion reactions like the burning of n-butanol are fundamental in energy production. When you use a butane lighter or burn fuels in an engine, chemical energy stored in the bonds of the fuel is released as heat and light. By understanding stoichiometry, scientists and engineers can determine the precise amount of air (oxygen) required to burn a fuel completely, maximizing efficiency and minimizing harmful byproducts like carbon monoxide.