To balance the equation for the oxidation of butene ([tex]\(C_4H_8\)[/tex]), let's go through the steps to ensure the conservation of atoms for each element on both sides of the equation:
Given unbalanced equation:
[tex]\[ C_4H_8 + 6 O_2 \rightarrow CO_2 + H_2O \][/tex]
1. Balance the Carbons:
- On the reactant side, we have 4 carbon atoms in [tex]\(C_4H_8\)[/tex].
- On the product side, each [tex]\(CO_2\)[/tex] molecule contains 1 carbon atom.
- Therefore, we need 4 molecules of [tex]\(CO_2\)[/tex] to balance the carbon atoms.
[tex]\[ C_4H_8 + 6 O_2 \rightarrow 4 CO_2 + H_2O \][/tex]
2. Balance the Hydrogens:
- On the reactant side, we have 8 hydrogen atoms in [tex]\(C_4H_8\)[/tex].
- On the product side, each [tex]\(H_2O\)[/tex] molecule contains 2 hydrogen atoms.
- Therefore, we need 4 molecules of [tex]\(H_2O\)[/tex] to balance the hydrogen atoms.
[tex]\[ C_4H_8 + 6 O_2 \rightarrow 4 CO_2 + 4 H_2O \][/tex]
3. Verify the Oxygens:
- On the reactant side, we have 6 molecules of [tex]\(O_2\)[/tex], which gives [tex]\(6 \times 2 = 12\)[/tex] oxygen atoms.
- On the product side, each [tex]\(CO_2\)[/tex] molecule contains 2 oxygen atoms, and each [tex]\(H_2O\)[/tex] molecule contains 1 oxygen atom.
- With 4 [tex]\(CO_2\)[/tex] molecules, we have [tex]\(4 \times 2 = 8\)[/tex] oxygen atoms from [tex]\(CO_2\)[/tex].
- With 4 [tex]\(H_2O\)[/tex] molecules, we have [tex]\(4 \times 1 = 4\)[/tex] oxygen atoms from [tex]\(H_2O\)[/tex].
- Thus, the total number of oxygen atoms on the product side is [tex]\(8 + 4 = 12\)[/tex], matching the reactant side.
Since the equation is now balanced, for each molecule of [tex]\(C_4H_8\)[/tex] that reacts, the balanced chemical equation produces 4 molecules of [tex]\(CO_2\)[/tex] and 4 molecules of [tex]\(H_2O\)[/tex].
Therefore, the correct answer is:
- Four carbon dioxide molecules and four water molecules
Hence, the answer is:
[tex]\[ \text{four carbon dioxide molecules and four water molecules} \][/tex]
