CH4+ 2O2--> CO2 + 2H2O

molecular mass of CO2= 12+2(16)
=12+32
=44


No. of moles required= 22/44
=0.5 mole

Calculating the Number of Methane Molecules

In order to determine the number of methane molecules required to produce 22g of CO2(g) after combustion, we can follow a step-by-step process.

Step 1: Identify the Balanced Chemical Equation
The balanced chemical equation for the combustion of methane (CH4) is as follows:
CH4 + 2O2 -> CO2 + 2H2O

Step 2: Determine the Molar Mass of CO2
The molar mass of CO2 can be calculated by adding up the atomic masses of carbon (C) and two oxygen (O) atoms.
Molar mass of CO2 = 12.01 g/mol (C) + 2 * 16.00 g/mol (O)
Molar mass of CO2 = 44.01 g/mol

Step 3: Calculate the Number of Moles of CO2
To find the number of moles of CO2 produced, we can use the equation:
Number of moles = Mass / Molar mass

Given that the mass of CO2 produced is 22g, we can substitute the values into the equation:
Number of moles of CO2 = 22g / 44.01 g/mol
Number of moles of CO2 ≈ 0.500 mol

Step 4: Determine the Stoichiometry
From the balanced chemical equation, we can see that one mole of methane (CH4) produces one mole of CO2. Therefore, the number of moles of methane consumed will be the same as the number of moles of CO2 produced.

Step 5: Calculate the Number of Molecules of Methane
To find the number of molecules, we need to use Avogadro's number, which states that one mole of any substance contains 6.022 × 10^23 particles (atoms, molecules, or formula units).

Number of molecules = Number of moles * Avogadro's number
Number of molecules = 0.500 mol * 6.022 × 10^23 molecules/mol
Number of molecules ≈ 3.011 × 10^23 molecules

Therefore, approximately 3.011 × 10^23 molecules of methane are required to produce 22g of CO2(g) after combustion.