An automobile gasoline tank holds 45 kg of gasoline. When the gasoline burns, 158 kg of oxygen are consumed and carbon dioxide and water are produced.What is the total combined mass of carbon dioxide and water that is produced?
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Using the coefficients of the balanced chemical equation:
2 moles of C8H18 react with 25 moles of O2 to produce 16 moles of CO2 and 18 moles of H2O.
So, if 158 kg of O2 is consumed, we can calculate the amount of gasoline used:
25 moles of O2 are needed for 2 moles of C8H18 to react.
158 kg of O2 is equal to (158/32) moles of O2.
So, the moles of C8H18 used would be (2/25) x (158/32) = 2.51 moles.
Using the same molar ratios, we can find the moles of CO2 produced:
16 moles of CO2 are produced for every 2 moles of C8H18 used.
So, the moles of CO2 produced would be (16/2) x 2.51 = 20.08 moles.
Similarly, we can find the moles of H2O produced:
18 moles of H2O are produced for every 2 moles of C8H18 used.
So, the moles of H2O produced would be (18/2) x 2.51 = 22.55 moles.
Now, we need to convert these moles into mass.
The molar mass of CO2 is 44 g/mol, so the mass of CO2 produced would be 20.08 x 44 = 883.52 g or 0.88352 kg.
The molar mass of H2O is 18 g/mol, so the mass of H2O produced would be 22.55 x 18 = 405.9 g or 0.4059 kg.
So, the total combined mass of carbon dioxide and water that is produced is 0.88352 kg + 0.4059 kg = 1.28942 kg, or approximately 1.29 kg.
To find the total combined mass of carbon dioxide and water produced when gasoline burns, we need to determine the amount of carbon dioxide and water produced from the given amounts of gasoline and oxygen.
Let's start by calculating the amount of carbon dioxide produced.
1. To burn gasoline, the balanced chemical equation is typically represented as:
C8H18 (Gasoline) + 12.5O2 (Oxygen) -> 8CO2 (Carbon dioxide) + 9H2O (Water)
2. From the equation, we see that for every 1 molecule of gasoline (C8H18), we need 12.5 molecules of oxygen (O2) to produce 8 molecules of carbon dioxide (CO2).
3. Given that the mass of gasoline is 45 kg, we can convert it to moles using the molar mass of gasoline, which is approximately 114.22 g/mol.
Moles of gasoline = Mass of gasoline / Molar mass of gasoline
= 45,000 g / 114.22 g/mol
≈ 394.02 mol
4. Using stoichiometry, we can determine the moles of carbon dioxide produced.
Moles of carbon dioxide = Moles of gasoline × (8 mol CO2 / 1 mol gasoline)
= 394.02 mol × (8 mol CO2 / 1 mol gasoline)
≈ 3152.16 mol
5. Finally, we convert moles of carbon dioxide to grams using the molar mass of carbon dioxide, which is approximately 44.01 g/mol.
Mass of carbon dioxide = Moles of carbon dioxide × Molar mass of carbon dioxide
= 3152.16 mol × 44.01 g/mol
≈ 138,661.08 g
≈ 138.66 kg
Next, let's calculate the mass of water produced.
1. Using the same balanced chemical equation, we see that for every 1 molecule of gasoline (C8H18), we produce 9 molecules of water (H2O).
2. Following the same steps as above, we can calculate the moles of water produced.
Moles of water = Moles of gasoline × (9 mol H2O / 1 mol gasoline)
= 394.02 mol × (9 mol H2O / 1 mol gasoline)
≈ 3,546.18 mol
3. Convert moles of water to grams using the molar mass of water (H2O), which is approximately 18.02 g/mol.
Mass of water = Moles of water × Molar mass of water
= 3,546.18 mol × 18.02 g/mol
≈ 63,920.04 g
≈ 63.92 kg
Therefore, the total combined mass of carbon dioxide and water produced from burning the given amount of gasoline and oxygen is approximately 138.66 kg (carbon dioxide) + 63.92 kg (water) = 202.58 kg.
gasoline is octane ... C8H18
2 C8H18 + 25 O2 ---> 16 CO2 + 18 H2O
the reaction equation gives the molar ratios
find the moles of O2 consumed, then calculate the moles of products produced