When butane \( \left(\mathrm{C}_{4} \mathrm{H}_{10}\right) \) is burnt in air, the resulting reaction liberates carbon dioxide and water. Which of the following describes this reaction? Choose 1 answer: (A) \( 2 \mathrm{C}_{4} \mathrm{H}_{10}+4 \mathrm{O}_{2} \rightarrow 2 \mathrm{CO}_{2}+4 \mathrm{H}_{2} \mathrm{O} \) (B) \( \mathrm{C}_{4} \mathrm{H}_{10}+5 \mathrm{O}_{2} \rightarrow 6 \mathrm{CO}_{2}+2 \mathrm{H}_{2} \mathrm{O} \) (C) \( 2 \mathrm{C}_{4} \mathrm{H}_{10}+13 \mathrm{O}_{2} \rightarrow 8 \mathrm{CO}_{2}+10 \mathrm{H}_{2} \mathrm{O} \) (D) \( \mathrm{C}_{4} \mathrm{H}_{10}+5 \mathrm{O}_{2} \rightarrow \mathrm{CO}_{2}+5 \mathrm{H}_{2} \mathrm{O} \)

When butane is burned in air, it reacts with oxygen to yield carbon dioxide and water through combustion. This reaction is characterized by the balancing of carbon, hydrogen, and oxygen atoms. Understanding the balanced chemical equation gives insight into how many molecules of each substance are involved in the process, providing a clear representation of the transformation of butane into energy-rich products. In practical applications, combustion reactions like that of butane are widespread, especially in household heating, cooking, and vehicles. By combusting butane in a controlled manner, we harness its energy while producing the necessary heat and light, demonstrating how chemistry underpins everyday life. However, it's vital to understand proper ventilation and safety measures since combustion produces carbon dioxide and potentially harmful pollutants.