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Answer :
Final answer:
The reaction between methane and oxygen produces 1.00 L of carbon dioxide and 2.00 L of water at STP.
Explanation:
The balanced chemical equation for the reaction between methane (CH4) and oxygen (O2) is:
CH4 + 2O2 → CO2 + 2H2O
From the balanced equation, we can see that for every 1 mole of methane, we get 1 mole of carbon dioxide and 2 moles of water. Since we're given the volume of methane as 1.00 L, we can assume it is at standard temperature and pressure (STP). At STP, 1 mole of any ideal gas occupies a volume of 22.4 L.
Therefore, 1.00 L of methane at STP corresponds to 1.00/22.4 = 0.0446 moles of methane. Using the stoichiometry of the balanced equation, we can determine the moles of carbon dioxide and water produced:
1 mole of methane produces 1 mole of carbon dioxide and 2 moles of water
0.0446 moles of methane will produce 0.0446 moles of carbon dioxide and 2(0.0446) = 0.0892 moles of water
Since 1 mole of any ideal gas occupies a volume of 22.4 L at STP, we can convert the moles to liters:
0.0446 moles of carbon dioxide is approximately 0.0446(22.4) = 1.00 L
0.0892 moles of water is approximately 0.0892(22.4) = 2.00 L
Therefore, the correct answer is (A) 1.00 L CO2 and 2.00 L H2O.
Learn more about Stoichiometry here:
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