Question

an organic compound contains carbon 62.15% and hydrogen 10.34% and molar mass 58 find empirical formula and molecular formula​

Answer 1

Answer:

$\bigstar{\bold{Empirical\:formula=CH_2}}$

$\bigstar{\bold{Molecular\:formula=C_4H_8}}$

Explanation:

$\Large{\underline{\underline{\bf{Given:}}}}$

• % of Carbon (C) = 62.15 %
• % of Hydrogen (H) = 10.34 %

$\Large{\underline{\underline{\bf{To\:Find:}}}}$

• Empirical formula
• Molecular formula

$\Large{\underline{\underline{\bf{Solution:}}}}$

→ First we have to find the number of moles of the two elements.

→ Number of moles of Carbon:

→ Number of moles of an element = Given mass/Molar mass

→ Number of moles of Carbon = 62.15/12

  Number of moles of Carbon = 5.18 moles

→ Number of moles of Hydrogen = 10.34/1

  Number of moles of Hydrogen = 10.34 moles

→ Now the whole number ratio of each element is given by

→ Simplest whole number ratio of Carbon = 5.18/5.18 = 1

→ Simplest whole number ratio of Hydrogen = 10.34/5.18 = 2

→ Empirical formula = CH₂

$\boxed{\bold{Empirical\:formula=CH_2}}$

→ Now we have to find the molecular mass of CH₂

  Molecular mass of CH₂ = 12 + 2 × 1

  Molecular mass of CH₂ = 12 + 2

  Molecular mass of CH₂ = 14

→ Now,

  Molar mass/Molecular formula = n

  58/14 = n

  n = 4

→ Now the molecular formula is given by

  n × Empirical formula = Molecular formula

  4 × (CH₂) = Molecular formula

 Molecular formula = C₄H₈

$\boxed{\bold{Molecular\:formula=C_4H_8}}$

$\Large{\underline{\underline{\bf{Notes:}}}}$

→ Number of moles = Given mass/Molar mass

→ n × Empirical formula = Molecular formula