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A 0.166 g sample of an organic compound was digested with conc. H2SO4 and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.
Correct answer is '63'. Can you explain this answer?
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A 0.166 g sample of an organic compound was digested with conc. H2SO4a...
Millimoles of used acid = 
Millimoles of NH3 = 30 × 0.25 = 7.5
Mass % of nitrogen =
≌ 63%
Millimoles of NH3 = 30 × 0.25 = 7.5
Mass % of nitrogen =
≌ 63%
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A 0.166 g sample of an organic compound was digested with conc. H2SO4a...
Mass of organic compound = 0.166 g
Volume of 0.5 N H2SO4 used = 50.0 mL = 0.050 L
Volume of 0.25 N NaOH used = 30.0 mL = 0.030 L
To find the mass percentage of nitrogen in the organic compound, we need to calculate the amount of nitrogen present in the compound.
Let's assume the organic compound has the formula CxHyNz. Since the compound contains nitrogen, we are interested in determining the value of z.
To calculate the amount of nitrogen, we can use the following equation:
Amount of nitrogen (in moles) = Volume of acid used (in L) × Normality of acid × Molar ratio between acid and nitrogen × Molar mass of nitrogen
In this case, the molar ratio between acid and nitrogen can be obtained from the balanced chemical equation for the neutralization reaction between H2SO4 and NaOH. The balanced equation is:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
From the equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaOH. Therefore, the molar ratio between H2SO4 and nitrogen is 1:2.
Now let's calculate the amount of nitrogen:
Amount of nitrogen = 0.050 L × 0.5 N × (1/2) × (14 g/mol)
Next, we can calculate the molar mass of the organic compound using the following equation:
Molar mass of compound = Mass of compound (in g) / Amount of compound (in moles)
Since we know the mass of the compound (0.166 g) and the amount of nitrogen (calculated above), we can rearrange the equation to solve for the molar mass of the compound.
Molar mass of compound = 0.166 g / (Amount of nitrogen + Molar mass of nitrogen)
Finally, we can calculate the mass percentage of nitrogen in the compound:
Mass percentage of nitrogen = (Amount of nitrogen × Molar mass of nitrogen) / Molar mass of compound × 100
Substituting the values into the equation:
Mass percentage of nitrogen = (0.050 L × 0.5 N × (1/2) × (14 g/mol) × 14 g/mol) / (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
Simplifying the equation:
Mass percentage of nitrogen = (0.050 L × 0.5 N × 7 g) / (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
Mass percentage of nitrogen = (0.175 g) / (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
Now, let's solve for the value of Amount of nitrogen:
0.175 g = (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
0.175 g / 100 = 0.166 g / (Amount of nitrogen + 14 g/mol)
1.75 = 0.166 / (Amount of nitrogen + 14)
1.75 × (Amount of nitrogen + 14) = 0.166
1.75 × Amount of nitrogen +
Volume of 0.5 N H2SO4 used = 50.0 mL = 0.050 L
Volume of 0.25 N NaOH used = 30.0 mL = 0.030 L
To find the mass percentage of nitrogen in the organic compound, we need to calculate the amount of nitrogen present in the compound.
Let's assume the organic compound has the formula CxHyNz. Since the compound contains nitrogen, we are interested in determining the value of z.
To calculate the amount of nitrogen, we can use the following equation:
Amount of nitrogen (in moles) = Volume of acid used (in L) × Normality of acid × Molar ratio between acid and nitrogen × Molar mass of nitrogen
In this case, the molar ratio between acid and nitrogen can be obtained from the balanced chemical equation for the neutralization reaction between H2SO4 and NaOH. The balanced equation is:
H2SO4 + 2NaOH → Na2SO4 + 2H2O
From the equation, we can see that 1 mole of H2SO4 reacts with 2 moles of NaOH. Therefore, the molar ratio between H2SO4 and nitrogen is 1:2.
Now let's calculate the amount of nitrogen:
Amount of nitrogen = 0.050 L × 0.5 N × (1/2) × (14 g/mol)
Next, we can calculate the molar mass of the organic compound using the following equation:
Molar mass of compound = Mass of compound (in g) / Amount of compound (in moles)
Since we know the mass of the compound (0.166 g) and the amount of nitrogen (calculated above), we can rearrange the equation to solve for the molar mass of the compound.
Molar mass of compound = 0.166 g / (Amount of nitrogen + Molar mass of nitrogen)
Finally, we can calculate the mass percentage of nitrogen in the compound:
Mass percentage of nitrogen = (Amount of nitrogen × Molar mass of nitrogen) / Molar mass of compound × 100
Substituting the values into the equation:
Mass percentage of nitrogen = (0.050 L × 0.5 N × (1/2) × (14 g/mol) × 14 g/mol) / (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
Simplifying the equation:
Mass percentage of nitrogen = (0.050 L × 0.5 N × 7 g) / (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
Mass percentage of nitrogen = (0.175 g) / (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
Now, let's solve for the value of Amount of nitrogen:
0.175 g = (0.166 g / (Amount of nitrogen + 14 g/mol)) × 100
0.175 g / 100 = 0.166 g / (Amount of nitrogen + 14 g/mol)
1.75 = 0.166 / (Amount of nitrogen + 14)
1.75 × (Amount of nitrogen + 14) = 0.166
1.75 × Amount of nitrogen +
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A 0.166 g sample of an organic compound was digested with conc. H2SO4and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.Correct answer is '63'. Can you explain this answer?
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A 0.166 g sample of an organic compound was digested with conc. H2SO4and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.Correct answer is '63'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A 0.166 g sample of an organic compound was digested with conc. H2SO4and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.Correct answer is '63'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 0.166 g sample of an organic compound was digested with conc. H2SO4and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.Correct answer is '63'. Can you explain this answer?.
A 0.166 g sample of an organic compound was digested with conc. H2SO4and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.Correct answer is '63'. Can you explain this answer? for JEE 2024 is part of JEE preparation. The Question and answers have been prepared according to the JEE exam syllabus. Information about A 0.166 g sample of an organic compound was digested with conc. H2SO4and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.Correct answer is '63'. Can you explain this answer? covers all topics & solutions for JEE 2024 Exam. Find important definitions, questions, meanings, examples, exercises and tests below for A 0.166 g sample of an organic compound was digested with conc. H2SO4and then distilled with NaOH. The ammonia gas evolved was passed through 50.0 mL of 0.5 N H2SO4. The used acid required 30.0 mL of 0.25 N NaOH for complete neutralisation. The mass percentage of nitrogen in the organic compound is ________.Correct answer is '63'. Can you explain this answer?.
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