Butane gas, C4H10, reacts with oxygen gas (O2) to produce carbon dioxide and water vapor. Write the balanced chemical reaction for this process.
The Correct Answer and Explanation is :
The combustion of butane ((C_4H_{10})) in the presence of oxygen gas ((O_2)) produces carbon dioxide ((CO_2)) and water vapor ((H_2O)). The balanced chemical reaction for this process is:
[
2 \, C_4H_{10} + 13 \, O_2 \rightarrow 8 \, CO_2 + 10 \, H_2O
]
Explanation
The reaction is an example of a combustion reaction, which involves a fuel reacting with an oxidizing agent (in this case, oxygen) to produce heat and light, typically in the form of flames. In this scenario, butane serves as the hydrocarbon fuel, commonly found in lighters and portable stoves.
- Balancing the Reaction:
- The first step in balancing the reaction is to identify the number of carbon, hydrogen, and oxygen atoms on both sides of the equation.
- Butane ((C_4H_{10})) contains 4 carbon atoms and 10 hydrogen atoms. Thus, when it combusts, it will produce (CO_2) (one carbon dioxide molecule contains one carbon atom) and (H_2O) (one water molecule contains two hydrogen atoms).
- Therefore, to balance the carbon, we need 8 (CO_2) molecules (since (2 \times 4 = 8)). To balance the hydrogen, we need 10 (H_2O) molecules (since (10 \div 2 = 5)).
- Oxygen Balancing:
- Next, we count the oxygen atoms produced on the right side.
- Each (CO_2) molecule contains 2 oxygen atoms, contributing a total of (8 \times 2 = 16) oxygen atoms. Each (H_2O) molecule contains 1 oxygen atom, contributing (10) oxygen atoms. Thus, the total oxygen atoms needed on the product side is (16 + 10 = 26).
- Since (O_2) is diatomic, we require (26 \div 2 = 13) (O_2) molecules to provide enough oxygen for the reaction.
- Final Verification:
- The balanced equation ensures that the number of each type of atom is the same on both sides, which is crucial for the law of conservation of mass. Thus, the reaction is balanced correctly.
In conclusion, this balanced equation depicts the stoichiometry of butane combustion, showcasing the transformation of chemical energy into thermal energy, which is harnessed for practical uses like cooking and heating.