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During estimation of nitrogen in the organic compound by Kjeldahl’s method, the ammonia evolved from 0.5 g of the compound in Kjeldahl’s estimation of nitrogen, neutralised 10 mL of 1M H2SO4.
Find out the percentage of nitrogen in the compound.
- a)14%
- b)28%
- c)56%
- d)68%
Correct answer is option 'C'. Can you explain this answer?
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Most Upvoted Answer
During estimation of nitrogen in the organic compound by Kjeldahl&rsqu...
Gm eq of acid =gm eq of ammoniaN×V (ml)/1000 =w/17find w I.e. of Nh3nowfrom kjeldal methodNh3of mw 17gives =14gm of nitrogenthen w gran gives=14/17×w Eq number 1mass percent of element =mass of element from equation1/ mass of organic compound given=1.4×2×10/0.5=56%REMEMBER if base is also given them gm eq of acid -gm eq of basewhile finding amount of ammonia
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During estimation of nitrogen in the organic compound by Kjeldahl&rsqu...
Understanding Kjeldahl's Method
Kjeldahl's method is widely used for determining nitrogen content in organic compounds. It involves converting nitrogen in the sample into ammonia, which is then quantified.
Calculating Moles of H2SO4
- Given: 10 mL of 1M H2SO4
- Moles of H2SO4 = Concentration (M) × Volume (L)
- Convert 10 mL to liters: 10 mL = 0.01 L
- Moles of H2SO4 = 1 mol/L × 0.01 L = 0.01 moles
Neutralization Reaction
- The neutralization of ammonia (NH3) with sulfuric acid (H2SO4) occurs as follows:
2 NH3 + H2SO4 → (NH4)2SO4
- From the reaction, 1 mole of H2SO4 neutralizes 2 moles of NH3. Therefore:
- Moles of NH3 = 2 × Moles of H2SO4
- Moles of NH3 = 2 × 0.01 = 0.02 moles
Calculating Mass of Nitrogen
- Molecular weight of nitrogen (N) = 14 g/mol
- Mass of nitrogen in 0.02 moles = 0.02 moles × 14 g/mol = 0.28 g
Determining Percentage of Nitrogen
- Percentage of Nitrogen = (Mass of N / Mass of compound) × 100
- Mass of the organic compound = 0.5 g
- Percentage of Nitrogen = (0.28 g / 0.5 g) × 100 = 56%
Conclusion
The percentage of nitrogen in the organic compound is 56%, confirming that the correct answer is option 'C'.
Kjeldahl's method is widely used for determining nitrogen content in organic compounds. It involves converting nitrogen in the sample into ammonia, which is then quantified.
Calculating Moles of H2SO4
- Given: 10 mL of 1M H2SO4
- Moles of H2SO4 = Concentration (M) × Volume (L)
- Convert 10 mL to liters: 10 mL = 0.01 L
- Moles of H2SO4 = 1 mol/L × 0.01 L = 0.01 moles
Neutralization Reaction
- The neutralization of ammonia (NH3) with sulfuric acid (H2SO4) occurs as follows:
2 NH3 + H2SO4 → (NH4)2SO4
- From the reaction, 1 mole of H2SO4 neutralizes 2 moles of NH3. Therefore:
- Moles of NH3 = 2 × Moles of H2SO4
- Moles of NH3 = 2 × 0.01 = 0.02 moles
Calculating Mass of Nitrogen
- Molecular weight of nitrogen (N) = 14 g/mol
- Mass of nitrogen in 0.02 moles = 0.02 moles × 14 g/mol = 0.28 g
Determining Percentage of Nitrogen
- Percentage of Nitrogen = (Mass of N / Mass of compound) × 100
- Mass of the organic compound = 0.5 g
- Percentage of Nitrogen = (0.28 g / 0.5 g) × 100 = 56%
Conclusion
The percentage of nitrogen in the organic compound is 56%, confirming that the correct answer is option 'C'.
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During estimation of nitrogen in the organic compound by Kjeldahl’s method, the ammonia evolved from 0.5 g of the compound in Kjeldahl’s estimation of nitrogen, neutralised 10 mL of 1M H2SO4.Find out the percentage of nitrogen in the compound.a)14%b)28%c)56%d)68%Correct answer is option 'C'. Can you explain this answer?
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