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How many moles of methane are required to produce 22g CO2(g) after combustion?
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Problem Statement:
How many moles of methane are required to produce 22g CO2(g) after combustion?

Solution:

Step 1: Balanced chemical equation
We need to start by writing the balanced chemical equation for the combustion of methane (CH4):

CH4 + 2O2 -> CO2 + 2H2O

This equation shows that one molecule of methane reacts with two molecules of oxygen to produce one molecule of carbon dioxide and two molecules of water.

Step 2: Molar mass
To find the number of moles, we need to calculate the molar mass of CO2. Carbon has a molar mass of 12.01 g/mol, and oxygen has a molar mass of 16.00 g/mol. Since carbon dioxide (CO2) has one carbon atom and two oxygen atoms, its molar mass is:

Molar mass of CO2 = (12.01 g/mol) + 2(16.00 g/mol) = 44.01 g/mol

Step 3: Conversion
Now we can use the molar mass of CO2 to convert the given mass (22g) into moles.

Number of moles = Mass (g) / Molar mass (g/mol)
Number of moles = 22g / 44.01 g/mol
Number of moles = 0.499 moles

Step 4: Stoichiometry
According to the balanced chemical equation, one mole of methane reacts to produce one mole of carbon dioxide. Therefore, the number of moles of methane required would also be 0.499 moles.

Answer:
Therefore, 0.499 moles of methane are required to produce 22g of CO2(g) after combustion.
Community Answer
How many moles of methane are required to produce 22g CO2(g) after com...
0.5 moles..
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How many moles of methane are required to produce 22g CO2(g) after combustion?
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