Chemistry, asked by jhameshtekam61, 5 months ago


calculate the empirical and molecular formula of the compound having t
following percentage composition:
C=26.59%. H=2.22% 0=71.19%, its molecular mass is 90.​

Answers

Answered by Ekaro
20

Given :

Per. composition of C = 26.59%

Per. composition of H = 2.22%

Per. composition of O = 71.19%

To Find :

Molecular and empirical formula of the compound.

Solution :

Atomic mass of C = 12g

Atomic mass of H = 1g

Atomic mass of O = 16g

\bullet\sf \ No. \ of \ moles \ of \ C = \dfrac{26.59}{12} = 2.22

\bullet\sf \ No. \ of \ moles \ of \ H= \dfrac{2.22}{1} = 2.22

\bullet\sf\ No \ of \ moles \ of \ O = \dfrac{71.79}{16} = 4.44

Simplest ratio :

\implies\sf \sf \dfrac{2.22}{2.22} \ : \ \dfrac{2.22}{2.22} \ : \ \dfrac{4.44}{2.22}

\implies\bf 1 \ : \ 1 \ : \ 2

\bigstar\:\underline{\boxed{\bf{\purple{Empirical\:Formula=CHO_2}}}}

Empirical formula mass :

  • C + H + 2(O)
  • 12 + 1 + 2(16)
  • 45

We know that,

\dag\:\bf Molecular \ formula = n \times Empirical\ formula

➠ n = Molar mass / Formula mass

➠ n = 90/45

n = 2

\bullet\sf\:Molecular\ formula=2\times CHO_2

\dag\:\underline{\boxed{\bf{\pink{Molecular\ Formula=C_2H_2O_4}}}}

Answered by amazingbuddy
13

\huge{\mathtt{\red{\underline {Given : }}}}

Percentage composition of C = 26.59%

Percentage composition of H = 2.22%

Percentage composition of O = 71.19%

\huge{\mathtt{\purple{\underline {To\: Find : }}}}

Molecular and empirical formula of the compound.

\huge{\mathtt{\pink{\underline {Solution : }}}}

Atomic mass of C = 12g

Atomic mass of H = 1g

Atomic mass of O = 16g

\bullet\sf \ No. \ of \ moles \ of \ C = \dfrac{26.59}{12} = 2.22.

\bullet\sf \ No. \ of \ moles \ of \ H= \dfrac{2.22}{1} = 2.22∙

\bullet\sf\ No \ of \ moles \ of \ O = \dfrac{71.79}{16} = 4.44∙

Simplest ratio :

:\implies\sf \sf \dfrac{2.22}{2.22} \ : \ \dfrac{2.22}{2.22} \ : \ \dfrac{4.44}{2.22}

:\implies\bf 1 \ : \ 1 \ : \ 2⟹1 : 1 : 2

{\boxed{\boxed{\bf{\orange{Empirical\:Formula=CHO_2}}}}}

We know that,

\dag\:\bf Molecular \ formula = n \times Empirical\ formula

\sf n = \dfrac {Molar\: mass }{Formula \:mass}

\sf n = \dfrac {90}{45}

★ n = 2 ★

\bullet\sf\:Molecular\ formula=2\times CHO_2.

{\boxed{\boxed{\bf{\blue{Molecular\ Formula=C_2H_2O_4}}}}}

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