Chemistry, asked by aalok1246, 10 months ago

13. A crystalline salt when heated becomes anhydrous
and loses 51.2% of its weight. The anhydrous salt
on analysis gave the following percentage
composition:
Mg = 20.0%, S = 26.66%, 0 = 53.33%
Calculate the molecular formula of the anhydrous
salt and the crystalline salt. Molecular weight of
the anhydrous salt is 120.​

Answers

Answered by ankita1508
112

Answer:

M

Explanation:

Mg = 20.0% ,S = 26.66% ,O = 53.33%.

suppose 100 mg of the compound is present. This changes the percentage to grams..

Mg = 20g , S = 26.66g , O = 53.33g

convert the masses to mole,

Mg = 20 /24 = 0.8333 moles

S = 26.66/ 32 = 0.8331 moles

O = 53.33 /16 = 3.3331 moles.

divide by lowest no .of moles

Mg = 0.8333/ 0.8331 = 1 , S = 0.8331 / 0.8331 = 1 , O = 3.3331 / 0.8331 = 1

Empirical formula = MgSO4

Molecular mass = 120

Molecular formula = MgSo4

As crystalline salt on becoming anhydrous losses 51.2% by mass , this means 48.8g of anhydrous salt contains H2O = 51.2g

Therefore, 120 mg of anhydrous salt contains H2O = (51.2 /48.8)× 120 = 126g

No.of molecules = 126 /18 = 7 molecules.

Hence, molecular formula of crystalline salt = MgSO4.7H2O.

Answered by Saiakshat29
7

Answer:

M

Explanation:

Mg = 20.0% ,S = 26.66% ,O = 53.33%.

suppose 100 mg of the compound is present. This changes the percentage to grams..

Mg = 20g , S = 26.66g , O = 53.33g

convert the masses to mole,

Mg = 20 /24 = 0.8333 moles

S = 26.66/ 32 = 0.8331 moles

O = 53.33 /16 = 3.3331 moles.

divide by lowest no .of moles

Mg = 0.8333/ 0.8331 = 1 , S = 0.8331 / 0.8331 = 1 , O = 3.3331 / 0.8331 = 1

Empirical formula = MgSO4

Molecular mass = 120

Molecular formula = MgSo4

As crystalline salt on becoming anhydrous losses 51.2% by mass , this means 48.8g of anhydrous salt contains H2O = 51.2g

Therefore, 120 mg of anhydrous salt contains H2O = (51.2 /48.8)× 120 = 126g

No.of molecules = 126 /18 = 7 molecules.

Hence, molecular formula of crystalline salt = MgSO4.7H2O.

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