Avogadro’s law states that one mole of an ideal gas takes up around liters at standard temperature and pressure. Assuming all reagents can be treated as ideal gases, how many grams of carbon dioxide are produced in the complete reaction of liters of butane ( ) with oxygen to produce carbon dioxide (at STP)?
Question
Avogadro’s law states that one mole of an ideal gas takes up around liters at standard temperature and pressure. Assuming all reagents can be treated as ideal gases, how many grams of carbon dioxide are produced in the complete reaction of liters of butane ( ) with oxygen to produce carbon dioxide (at STP)?
Solution
To solve this problem, we need to follow these steps:
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According to Avogadro's law, 1 mole of any gas at standard temperature and pressure (STP) occupies 22.4 liters. So, first we need to find out how many moles of butane are there in 2.5 liters. We can do this by dividing the volume of butane by the volume occupied by one mole of gas at STP.
Moles of butane = 2.5 liters / 22.4 liters/mole = 0.111 moles
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The balanced chemical equation for the reaction of butane with oxygen is:
2C4H10 + 13O2 -> 8CO2 + 10H2O
From this equation, we can see that 2 moles of butane produce 8 moles of carbon dioxide. Therefore, 0.111 moles of butane will produce:
Moles of CO2 = 0.111 moles * (8 moles CO2 / 2 moles C4H10) = 0.444 moles of CO2
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The molar mass of carbon dioxide (CO2) is approximately 44.01 g/mole. So, the mass of carbon dioxide produced in the reaction is:
Mass of CO2 = 0.444 moles * 44.01 g/mole = 19.54 grams
So, approximately 19.54 grams of carbon dioxide are produced in the complete reaction of 2.5 liters of butane with oxygen to produce carbon dioxide (at STP).
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