Question

What is the volume (in litres) of oxygen at STP required for complete combustion of \[32\] g of \[C{{H}_{4}}\] ? [Molecular Weight of \[C{{H}_{4}}\] is \[16\] ].
A.$44.8$
B.$89.6$
C.$22.4$
D.$179.2$

Answer 1

Hint: We know that combustion is a process in which a substance reacts with oxygen from the air. When complete combustion of methane in presence of oxygen produces carbon dioxide and water. The balanced chemical equation for the reaction is: $C{{H}_{4}}+2{{O}_{2}}\to C{{O}_{2}}+2{{H}_{2}}O.$

Complete answer:
As we know that the combustion of organic products completely combustion always produces carbon dioxide and water. Therefore, in order to solve this question, write the balanced equation for reaction of ethylene and oxygen and use its stoichiometric coefficients to find the weight. Also, the Stoichiometry is defined as the exact numbers which indicate the actual proportions of the reactant and product.
Combustion is also known as burning. It is a high-temperature exothermic redox chemical reaction. Combustion is a process in which a substance reacts with oxygen from the air. It is an exothermic reaction and is of two types that are incomplete and complete combustion. The products formed when complete combustion of a hydrocarbon takes place are carbon dioxide and water. The moles of \[C{{H}_{4}}=\dfrac{32}{16}=2mol.\] Thus for two mole of methane we require four moles of oxygen and the volume of one mole of oxygen at STP is $22.4L$ along with volume of four moles of oxygen at STP is $4\times 22.4=89.6L.$
Therefore, the correct answer is option B.

Note:
Remember that the carbon dioxide and other products of combustion are greenhouse gases that trap solar radiation and increase the temperature of the earth, leading to a serious problem called global warming.