The balanced equation for the combustion of butane is: 2C4H10+13O2 8CO2+10H2O
The correct answer and explanation is :
The balanced chemical equation for the combustion of butane (( C_4H_{10} )) is:
[
2C_4H_{10} + 13O_2 \rightarrow 8CO_2 + 10H_2O
]
Explanation:
Combustion is a chemical reaction in which a substance reacts with oxygen, releasing energy in the form of heat and light. Butane (( C_4H_{10} )), a hydrocarbon, undergoes complete combustion in the presence of excess oxygen (( O_2 )), producing carbon dioxide (( CO_2 )) and water (( H_2O )).
Step-by-Step Balancing:
- Carbon Atoms: Butane has 4 carbon atoms per molecule. Since 2 molecules of butane are involved, we need ( 2 \times 4 = 8 ) carbon atoms in the products. This means 8 molecules of ( CO_2 ) are needed.
- Hydrogen Atoms: Each butane molecule has 10 hydrogen atoms. Since we have 2 molecules, there are ( 2 \times 10 = 20 ) hydrogen atoms. To balance this, we need 10 molecules of ( H_2O ) (since each water molecule contains 2 hydrogen atoms).
- Oxygen Atoms: On the right side, there are ( 8 \times 2 = 16 ) oxygen atoms from ( CO_2 ) and ( 10 \times 1 = 10 ) oxygen atoms from ( H_2O ), totaling 26 oxygen atoms. To balance this, we need 13 molecules of ( O_2 ) (since each molecule contains 2 oxygen atoms, giving ( 13 \times 2 = 26 ) oxygen atoms).
Thus, the equation is balanced:
( 2C_4H_{10} + 13O_2 \rightarrow 8CO_2 + 10H_2O )
Importance:
- Complete combustion ensures maximum energy output and minimal pollution.
- Incomplete combustion occurs with limited oxygen, producing carbon monoxide (( CO )), a toxic gas.
- This reaction is commonly used in lighters, stoves, and gas heaters.
