A compound contains H=4.07%, c=24.47%and Ci=71.65% its molar mass is 99gram/mol find the molecular formula of its compound
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GIVEN:
- Percentage composition of Hydrogen in the compound is 4.07 %
- Percentage composition of Carbon in the compound is 24.47 %
- Percentage composition of Chlorine in the compound is 71.65 %
⠀⠀⠀Molar mass = 99 g/mol
TO FIND:
Molecular formula of the compound
SOLUTION:
Strep 1 : Calculating relative number of atoms
⠀⠀⠀⠀a. Hydrogen
- Percentage composition = 4.07 %
- Atomic weight of hydrogen = 1
- Relative number of atoms = = 4.07
⠀⠀⠀⠀b. Carbon
- Percentage comppsition = 24.47 %
- Aomic weight of carbon = 12
- Relative number of atoms = = 2.02
⠀⠀⠀⠀c. Chlorine
- Percentage comppsition = 71.65%
- Atomic weight of chlorine = 35.5
- Relative number of atoms = = 2.01
Step 2 : Calculating Simplest ratio for each element
Simplest ratio is calculted by dividing all the values we got by the smallest value we got.
The smallest value we got is 2.01
⠀⠀⠀a. Hydrogen
Simplest ratio = 2
⠀⠀⠀b. Carbon
Simplest ratio = 1
⠀⠀⠀c. Chlorine
- Simplest ratio = = 1
- The empirical formula becomes CH₂Cl
- Molecular weight of Empirical formula = 12 + 2(1) + 35.5 = 49.5
- We are already given that molecular weight as 99.
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Relation between Empirical formula and Molecular formula is given by ,
n is some integer which is given by ,
We know the values for calculating the value of n . So , by substituting we get ;
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Applying the first formulae , (i.e , relation between empirical formulae and Molecular formulae) we get ;
Hence , The molecular formula of the given compound is C₂H₄Cl₂
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Answer:
compound contains H=4.07%, c=24.47%and Ci=71.65% its molar mass is
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