A compound has the following percentage composition by mass: carbon 14.4%,hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. [H = 1;C=12;Cl = 35.5]

CHCl₂

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CHCl

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CHCl₄

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CH₃Cl

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Solution

The correct option is A
CHCl₂

$\begin{matrix} E l e m e n t & % c o m p o s i t i o n & A t . W t, & A t o m i c r a t i o & S i m p l e s t a t o m i c r a t i o C a r b o n & 14.4 & 12 & \frac{14.4}{12} = 1.2 & \frac{1.2}{1.2} = 1 H y d r o g e n & 1.2 & 1 & \frac{1.2}{1} = 1.2 & \frac{1.2}{1.2} = 1 C h l o r i n e & 84.5 & 35.5 & \frac{84.5}{35.5} = 2.4 & \frac{2.4}{1.2} = 2 \end{matrix}$

Hence, the empirical formula of the compound is $C H C l_{2}$ .

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Similar questions

Q. A compound contains carbon 14.4 %, hydrogen 1.2 % and chlorine 84.5 %. The relative molecular mass of this compound is 168, its molecular formula is:

[C = 12, H = 1, C l = 35.5]

(a) from the equation"
$C + 2 H_{2} S O_{4} \to C O_{2} + 2 H_{2} O + 2 S O_{2}$
Calculate:
(i) hte mass of carbon oxidized by 49 g of sulphuric acid.
(ii) the volume of sulphur dioxide measured at STP, linerated at the same time.
(b) (i) A compound has the following percentage composition by mass; carbon 14.4 % hydrogen 1.2% and chlorine 84.5 % . Determine the empirical formula of this compound. Work correct to 1 decimal place. (H - 1; C = 12; Cl = 35.5)
(ii) The relativ molecular mass of this compound is 168, so what is its molecular formuka?

A compound has the following percentage composition by mass-

Carbon-14.4%

Hydrogen-1.2%

Chlorine-85.5%

The relative molecular mass of this compound is 168.50 what ia is molecular formula?

(a) (i) A compound has the following percentage composition by mass: carbon 14.4%, hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. Work correct to 1 decimal place. (H = 1; C = 12; Cl = 35.5)
(ii) The relative molecular mass of this compound is 168, so what is its molecular formula?
(iii) By what type of reaction could this compound be obtained from ethyne?

(b) From the equation:
C + 2H₂SO₄ $\overset{}{\to}$ CO₂ + 2H₂O + 2SO₂
Calculate:
(i) the mass of carbon oxidised by 49 g of sulphuric acid (C = 12; relative molecular mass of sulphuric acid = 98).
(ii) the volume of sulphur dioxide measured at STP, liberated at the same time.
(Volume occupied by 1 mole of a gas at STP is 22.4 dm³).

Q. A carbon compound on analysis gives the following percentage composition. Carbon

14.5

, hydrogen

1.8

chlorine

64.6

, oxygen

19.24

. The empirical formula of the compound is:

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A compound has the following percentage composition by mass: carbon 14.4%,hydrogen 1.2% and chlorine 84.5%. Determine the empirical formula of this compound. [H = 1;C=12;Cl = 35.5]

The correct option is A CHCl2 Element% compositionAt.Wt,Atomic ratioSimplest atomic ratioCarbon14.41214.412=1.21.21.2=1Hydrogen1.211.21=1.21.21.2=1Chlorine84.535.584.535.5=2.42.41.2=2 Hence, the empirical formula of the compound is CHCl2.