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Standard XII

Chemistry

Mole Concept

The molecular...

Question

The molecular mass of butyric acid was determined by experiment to be 88 $g m o l^{- 1}$ . What is the molecular formula?
Empirical formula=. $C_{2} H_{4} O$

C_{4} H_{8} O_{2}

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C_{2} H_{4} O

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C H_{4} O

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C_{2} H_{4} O_{2}

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Solution

The correct option is A $C_{4} H_{8} O_{2}$
Empirical formula mass $= 44$
Molecular mass $= 88$
we know,
$\frac{Molecular mass}{Empirical mass} = \frac{88}{44} = 2$
$∴ Molecular formula =Empirical formula \times n = C_{4} H_{8} O_{2}$

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Similar questions

Q. The molecular mass of butyric acid was determined by experiment to be 88

g m o l^{- 1}

. What is the molecular formula?
Empirical formula=.

C_{2} H_{4} O

Q. Butyric acid contains only

C, H

and

O

. A 4.24 mg sample of butyric acid is completely burned. It gives 8.45 mg of carbon dioxide

(C O_{2})

and 3.46 mg of water. What is the mass percentage of each element in butyric acid?The molecular mass of butyric acid was determined by experiment to be88. What is the molecular formula?

Butyric acid contains only C,H,O. A 4.24mg sample of butyric acid is completely burnt. It gives 8.45mg of CO2 and 3.46mg of H2O. What is the mass percentage of each element in butyric acid? The molecular mass of butyric acid was determined by experiment to be 88 a.m.u. What is the molecular formula?

Please help me solve this question briefly!!!

Q. Empirical formula = C₂H₄O
n=2
(n=molecular mass ÷ emperical formula mass
Emperical formula mass = 44
Molecular mass = 88)
molecular formula = n × empirical formula
= 2 × C₂H₄O
= C₄H₈O₂
but the book answer is given that C₄H₈O
Which is correct ? If the book answer is correct , tell me how ?

Q. The empirical formula of a compound is

C_{2} H_{4} O

. If the empirical formula mass is equal to one half of its vapor density, find the gram molecular mass of the compound.

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Mole Concept

Standard XII Chemistry

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The molecular mass of butyric acid was determined by experiment to be 88 gmol−1. What is the molecular formula? Empirical formula=.C2H4O

The correct option is A C4H8O2Empirical formula mass =44 Molecular mass =88 we know, Molecular massEmpirical mass=8844=2 ∴Molecular formula =Empirical formula× n=C4H8O2

The molecular mass of butyric acid was determined by experiment to be 88 $g m o l^{- 1}$ . What is the molecular formula?
Empirical formula=. $C_{2} H_{4} O$

The correct option is A $C_{4} H_{8} O_{2}$
Empirical formula mass $= 44$
Molecular mass $= 88$
we know,
$\frac{Molecular mass}{Empirical mass} = \frac{88}{44} = 2$
$∴ Molecular formula =Empirical formula \times n = C_{4} H_{8} O_{2}$