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1.6 g of an organic compound gave 2.6 g of magnesium pyrophosphate. The percentage of phosphorus in the compound is
- a)45.38%
- b)54.38%
- c)37.76%
- d)19.02%
Correct answer is option 'A'. Can you explain this answer?
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1.6 g of an organic compound gave 2.6 g of magnesium pyrophosphate. Th...
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Understanding the Problem
To find the percentage of phosphorus in the organic compound, we need to analyze the formation of magnesium pyrophosphate (Mg2P2O7) and the data provided.
Step 1: Calculate moles of magnesium pyrophosphate
- Molecular weight of Mg2P2O7:
- Mg: 24.31 g/mol (2 Mg = 48.62 g)
- P: 30.97 g/mol (2 P = 61.94 g)
- O: 16.00 g/mol (7 O = 112.00 g)
- Total: 48.62 + 61.94 + 112.00 = 222.56 g/mol
- Moles of Mg2P2O7 produced from 2.6 g:
- Moles = mass / molar mass = 2.6 g / 222.56 g/mol ≈ 0.0117 moles
Step 2: Calculate moles of phosphorus
- Each mole of Mg2P2O7 contains 2 moles of phosphorus (P).
- Moles of phosphorus = 2 × 0.0117 ≈ 0.0234 moles
Step 3: Calculate the mass of phosphorus
- Mass of phosphorus = moles × atomic weight
- Atomic weight of P = 30.97 g/mol
- Mass of phosphorus = 0.0234 moles × 30.97 g/mol ≈ 0.726 g
Step 4: Calculate percentage of phosphorus in the organic compound
- Percentage = (mass of phosphorus / mass of compound) × 100
- Percentage = (0.726 g / 1.6 g) × 100 ≈ 45.38%
Conclusion
The percentage of phosphorus in the organic compound is approximately 45.38%, which corresponds to option 'A'.
To find the percentage of phosphorus in the organic compound, we need to analyze the formation of magnesium pyrophosphate (Mg2P2O7) and the data provided.
Step 1: Calculate moles of magnesium pyrophosphate
- Molecular weight of Mg2P2O7:
- Mg: 24.31 g/mol (2 Mg = 48.62 g)
- P: 30.97 g/mol (2 P = 61.94 g)
- O: 16.00 g/mol (7 O = 112.00 g)
- Total: 48.62 + 61.94 + 112.00 = 222.56 g/mol
- Moles of Mg2P2O7 produced from 2.6 g:
- Moles = mass / molar mass = 2.6 g / 222.56 g/mol ≈ 0.0117 moles
Step 2: Calculate moles of phosphorus
- Each mole of Mg2P2O7 contains 2 moles of phosphorus (P).
- Moles of phosphorus = 2 × 0.0117 ≈ 0.0234 moles
Step 3: Calculate the mass of phosphorus
- Mass of phosphorus = moles × atomic weight
- Atomic weight of P = 30.97 g/mol
- Mass of phosphorus = 0.0234 moles × 30.97 g/mol ≈ 0.726 g
Step 4: Calculate percentage of phosphorus in the organic compound
- Percentage = (mass of phosphorus / mass of compound) × 100
- Percentage = (0.726 g / 1.6 g) × 100 ≈ 45.38%
Conclusion
The percentage of phosphorus in the organic compound is approximately 45.38%, which corresponds to option 'A'.
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1.6 g of an organic compound gave 2.6 g of magnesium pyrophosphate. The percentage of phosphorus in the compound isa)45.38%b)54.38%c)37.76%d)19.02%Correct answer is option 'A'. Can you explain this answer?
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