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An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?
- a)21.6%
- b)7.2%
- c)1.7%
- d)24.8%
Correct answer is option 'B'. Can you explain this answer?
Most Upvoted Answer
An impure sample of silver (1.5 g) is heated with S to form 0.124 g of...
216 g of Ag forms 248 g of Ag2S
1.5 g of Ag forms 248/216 x 1.5 = 1.722 g of Ag2S
% yield of Ag2S = 0.124/1.722 x 100 = 7.2%
1.5 g of Ag forms 248/216 x 1.5 = 1.722 g of Ag2S
% yield of Ag2S = 0.124/1.722 x 100 = 7.2%
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An impure sample of silver (1.5 g) is heated with S to form 0.124 g of...
**Given:**
- Mass of impure silver sample = 1.5 g
- Mass of Ag2S formed = 0.124 g
**To find:**
- Percentage yield of Ag2S
**Solution:**
**Step 1: Calculate the moles of Ag2S formed**
- The molar mass of Ag2S = 2(107.87 g/mol) + 32.06 g/mol = 232.8 g/mol
- Moles of Ag2S formed = Mass of Ag2S formed / Molar mass of Ag2S
= 0.124 g / 232.8 g/mol
≈ 0.00053 mol
**Step 2: Calculate the moles of silver used**
- The molar mass of silver (Ag) = 107.87 g/mol
- Moles of Ag used = Mass of silver used / Molar mass of Ag
= 1.5 g / 107.87 g/mol
≈ 0.0139 mol
**Step 3: Calculate the theoretical yield of Ag2S**
- The balanced chemical equation for the reaction is:
2Ag + S → Ag2S
- From the balanced equation, we can see that the ratio of moles of Ag2S formed to moles of Ag used is 1:2.
- Therefore, the moles of Ag2S formed would be twice the moles of Ag used.
- Theoretical yield of Ag2S = 2 * Moles of Ag used
= 2 * 0.0139 mol
= 0.0278 mol
**Step 4: Calculate the percentage yield**
- Percentage yield = (Actual yield / Theoretical yield) * 100
= (0.00053 mol / 0.0278 mol) * 100
≈ 1.91%
The calculated percentage yield is approximately 1.91%, which is closest to option C) 1.7%. However, none of the given options match the calculated percentage yield exactly. Therefore, the correct answer is not provided in the options given.
- Mass of impure silver sample = 1.5 g
- Mass of Ag2S formed = 0.124 g
**To find:**
- Percentage yield of Ag2S
**Solution:**
**Step 1: Calculate the moles of Ag2S formed**
- The molar mass of Ag2S = 2(107.87 g/mol) + 32.06 g/mol = 232.8 g/mol
- Moles of Ag2S formed = Mass of Ag2S formed / Molar mass of Ag2S
= 0.124 g / 232.8 g/mol
≈ 0.00053 mol
**Step 2: Calculate the moles of silver used**
- The molar mass of silver (Ag) = 107.87 g/mol
- Moles of Ag used = Mass of silver used / Molar mass of Ag
= 1.5 g / 107.87 g/mol
≈ 0.0139 mol
**Step 3: Calculate the theoretical yield of Ag2S**
- The balanced chemical equation for the reaction is:
2Ag + S → Ag2S
- From the balanced equation, we can see that the ratio of moles of Ag2S formed to moles of Ag used is 1:2.
- Therefore, the moles of Ag2S formed would be twice the moles of Ag used.
- Theoretical yield of Ag2S = 2 * Moles of Ag used
= 2 * 0.0139 mol
= 0.0278 mol
**Step 4: Calculate the percentage yield**
- Percentage yield = (Actual yield / Theoretical yield) * 100
= (0.00053 mol / 0.0278 mol) * 100
≈ 1.91%
The calculated percentage yield is approximately 1.91%, which is closest to option C) 1.7%. However, none of the given options match the calculated percentage yield exactly. Therefore, the correct answer is not provided in the options given.
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An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer?.
An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer? for NEET 2025 is part of NEET preparation. The Question and answers have been prepared according to the NEET exam syllabus. Information about An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer? covers all topics & solutions for NEET 2025 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer?.
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An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer?, a detailed solution for An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer? has been provided alongside types of An impure sample of silver (1.5 g) is heated with S to form 0.124 g of Ag2S. What was the per cent yield of Ag2S?a)21.6%b)7.2%c)1.7%d)24.8%Correct answer is option 'B'. Can you explain this answer? theory, EduRev gives you an
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