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A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?
- a)XCo2 = 0.176, XH2O = 0.235, XO2 = 0.588
- b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176
- c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588
- d)mole fraction of each component are similar
Correct answer is option 'A'. Can you explain this answer?
Verified Answer
A sample of propane (C3H8) placed in a closed vessel together with an ...
Let initially'm' mole of propane present when reaction is complete then
nO2 =15 m mol
When reaction is complete then
∴
Most Upvoted Answer
A sample of propane (C3H8) placed in a closed vessel together with an ...
To solve this problem, we need to determine the mole fraction of each component in the resulting mixture after the oxidation of propane to carbon dioxide (CO2) and water (H2O).
Given:
- The amount of O2 is three times the amount needed to completely oxidize the propane.
Let's assume we have 1 mole of propane (C3H8) for simplicity.
1. Determine the stoichiometry of the reaction:
The balanced equation for the complete combustion of propane is:
C3H8 + 5O2 -> 3CO2 + 4H2O
From the equation, we can see that for every mole of propane, we need 5 moles of O2 to completely react. However, we are given that the amount of O2 is three times the amount needed. Therefore, we have 3 * 5 = 15 moles of O2.
2. Calculate the moles of each component in the resulting mixture:
Since we have 1 mole of propane, we have:
- 1 mole of C3H8
- 15 moles of O2 (given)
- 3 moles of CO2 (from the stoichiometry of the reaction)
- 4 moles of H2O (from the stoichiometry of the reaction)
3. Calculate the total moles of the resulting mixture:
The total moles of the resulting mixture is the sum of the moles of each component:
Total moles = 1 + 15 + 3 + 4 = 23 moles
4. Calculate the mole fraction of each component:
Mole fraction (X) is calculated by dividing the moles of a component by the total moles of the mixture.
- Mole fraction of CO2 (XCO2) = moles of CO2 / total moles = 3 / 23 ≈ 0.130
- Mole fraction of H2O (XH2O) = moles of H2O / total moles = 4 / 23 ≈ 0.174
- Mole fraction of O2 (XO2) = moles of O2 / total moles = 15 / 23 ≈ 0.652
Therefore, the correct answer is option 'A':
a) XCo2 = 0.176, XH2O = 0.235, XO2 = 0.588
Given:
- The amount of O2 is three times the amount needed to completely oxidize the propane.
Let's assume we have 1 mole of propane (C3H8) for simplicity.
1. Determine the stoichiometry of the reaction:
The balanced equation for the complete combustion of propane is:
C3H8 + 5O2 -> 3CO2 + 4H2O
From the equation, we can see that for every mole of propane, we need 5 moles of O2 to completely react. However, we are given that the amount of O2 is three times the amount needed. Therefore, we have 3 * 5 = 15 moles of O2.
2. Calculate the moles of each component in the resulting mixture:
Since we have 1 mole of propane, we have:
- 1 mole of C3H8
- 15 moles of O2 (given)
- 3 moles of CO2 (from the stoichiometry of the reaction)
- 4 moles of H2O (from the stoichiometry of the reaction)
3. Calculate the total moles of the resulting mixture:
The total moles of the resulting mixture is the sum of the moles of each component:
Total moles = 1 + 15 + 3 + 4 = 23 moles
4. Calculate the mole fraction of each component:
Mole fraction (X) is calculated by dividing the moles of a component by the total moles of the mixture.
- Mole fraction of CO2 (XCO2) = moles of CO2 / total moles = 3 / 23 ≈ 0.130
- Mole fraction of H2O (XH2O) = moles of H2O / total moles = 4 / 23 ≈ 0.174
- Mole fraction of O2 (XO2) = moles of O2 / total moles = 15 / 23 ≈ 0.652
Therefore, the correct answer is option 'A':
a) XCo2 = 0.176, XH2O = 0.235, XO2 = 0.588
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A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer? for Chemistry 2025 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Chemistry 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer?.
A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer? for Chemistry 2025 is part of Chemistry preparation. The Question and answers have been prepared according to the Chemistry exam syllabus. Information about A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer? covers all topics & solutions for Chemistry 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer?.
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A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer?, a detailed solution for A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer? has been provided alongside types of A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer? theory, EduRev gives you an
ample number of questions to practice A sample of propane (C3H8) placed in a closed vessel together with an amount of O2, that is 3-times the amount needed to completely oxidize the propane to CO2 and H2O at constant temperature. Calculate the mole of fraction of each component in the resulting mixture after oxidation assuming that the H2O is present as a gas?a)XCo2 = 0.176,XH2O = 0.235, XO2 = 0.588b)XCo2 = 0.588, XH2O = 0.235, XO2 = 0.176c)XCo2 = 0.235, XH2O = 0.176, XO2 = 0.588d)mole fraction of each component are similarCorrect answer is option 'A'. Can you explain this answer? tests, examples and also practice Chemistry tests.
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