QuestionMay 27, 2025

C_(4)H_(9)OH+6O_(2)arrow 4CO_(2)+5H_(2)O

C_(4)H_(9)OH+6O_(2)arrow 4CO_(2)+5H_(2)O
C_(4)H_(9)OH+6O_(2)arrow 4CO_(2)+5H_(2)O

Solution
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Answer

The balanced equation is C_{4}H_{9}OH + 6O_{2} \rightarrow 4CO_{2} + 5H_{2}O. Explanation 1. Identify the type of reaction This is a combustion reaction where butanol (C_{4}H_{9}OH) reacts with oxygen (O_{2}). 2. Balance carbon atoms There are 4 carbon atoms in C_{4}H_{9}OH, so we need 4 CO_{2} molecules on the product side. 3. Balance hydrogen atoms There are 10 hydrogen atoms in C_{4}H_{9}OH, so we need 5 H_{2}O molecules on the product side. 4. Balance oxygen atoms Total oxygen atoms needed on the product side = 4 \times 2 + 5 \times 1 = 13. Since there are already 1 oxygen atom in C_{4}H_{9}OH, we need 12 more from O_{2}, which requires 6 O_{2} molecules.

Explanation

1. Identify the type of reaction<br /> This is a combustion reaction where butanol ($C_{4}H_{9}OH$) reacts with oxygen ($O_{2}$).<br /><br />2. Balance carbon atoms<br /> There are 4 carbon atoms in $C_{4}H_{9}OH$, so we need 4 $CO_{2}$ molecules on the product side.<br /><br />3. Balance hydrogen atoms<br /> There are 10 hydrogen atoms in $C_{4}H_{9}OH$, so we need 5 $H_{2}O$ molecules on the product side.<br /><br />4. Balance oxygen atoms<br /> Total oxygen atoms needed on the product side = $4 \times 2 + 5 \times 1 = 13$. Since there are already 1 oxygen atom in $C_{4}H_{9}OH$, we need $12$ more from $O_{2}$, which requires $6$ $O_{2}$ molecules.
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