Question
Download Solution PDFFor burning of 2 kilograms of methane (CH4) completely, the minimum number of kilograms of oxygen needed is (take atomic weight of H, C and O as 1, 12 and 16 respectively)
Answer (Detailed Solution Below)
Detailed Solution
Download Solution PDFExplanation:
Combustion of Methane
Definition: The combustion of methane (CH4) is a chemical reaction in which methane reacts with oxygen (O2) to produce carbon dioxide (CO2) and water (H2O). This reaction is exothermic, releasing energy in the form of heat and light. The balanced chemical equation for the complete combustion of methane is as follows:
CH4 + 2O2 → CO2 + 2H2O
Calculation: To determine the minimum number of kilograms of oxygen needed for the complete combustion of 2 kilograms of methane, let us follow a step-by-step approach:
Thus, the molecular weight of methane is 16 g/mol and that of oxygen is 32 g/mol.
From the balanced chemical equation:
1 mole of CH4 reacts with 2 moles of O2.
This means that 16 g of CH4 requires 2 × 32 = 64 g of O2 for complete combustion.
The mass ratio of CH4 to O2 is:
16 g CH4 : 64 g O2 = 1 : 4
For 2 kg (2000 g) of CH4, the amount of O2 required is:
2000 g CH4 × (4 g O2 / 1 g CH4) = 8000 g O2
Converting grams to kilograms:
8000 g O2 = 8 kg O2
The minimum number of kilograms of oxygen needed for the complete combustion of 2 kilograms of methane is 8 kg.
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