Question

0.13 9 gram of an organic compound gives 0.30 8 gram O2 and 0.08 1 gram of water on combustion when 0.20 85 gram of the organic compound is heated with any the liberated Ammonia needs 15 ml of an upon 20 H2 s o4 for complete neutralization calculate the percentage of c h n o in the compound​

Answer 1

ANSWER

Mass of organic compound = 0.50 g

60 mL of 0.5 M solution of NaOH is required by residual acid for neutralisation

⇒ 60 mL of 0.5 M solution of NaOH =260

mL of 0.5M H 2

SO 4

= 30mL of 0.5M H 2

SO 4

∴ Acid consumed in absorption of evolved ammonia is (50-30)mL = 20mL

Again, 20mL of 0.5M H 2

SO 4

= 40mL of 0.5M NH 3

Since 1000mL of 1M NH 3

contains 14g of nitrogen,

∴ 40mL of 0.5M NH 3

will contain = 1000

14×40

×0.5 = 0.28g of N

Therefore, percentage of N in 0.50g of organic compound =

0.50

0.28

×100=56%

Hence, the correct answer is 56%.

Explanation:

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