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

C_{2} H_{2} C l_{3}

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C_{2} H_{4} C l_{4}

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C H_{2} C l_{4}

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C_{2} H_{2} C l_{4}

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Solution

The correct option is D $C_{2} H_{2} C l_{4}$
Element % composition Atomic weight Relative No. of atoms Simplest ratio
Carbon 14.4 12 14.4/12 = 1.2 1.2/1.2 = 1
Hydrogen 1.2 1 1.2/1 = 1.2 1.2/1.2 = 1
Chlorine 84.5 35.5 84.5/35.5 = 2.38 2.38/1.2 = 2
Hence, empirical formula is $C H C l_{2}$ .
n = Molecular mass/Empirical formula mass
= 168/(12 + 1 + 70)
= 168/83
= 2.
Therefore, molecular formula $= (C H C l_{2}) \times 2 = C_{2} H_{2} C l_{4}$ .

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Similar questions

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]

(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 compound contains

4.07

% hydrogen,

24.27

% carbon and

71.65

% chlorine. It molar mass is

98 g

. What are its empirical and molecular formulas? (Atomic mass of C=12,H=1,Cl=35)

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Element	% composition	Atomic weight	Relative No. of atoms	Simplest ratio
Carbon	14.4	12	14.4/12 = 1.2	1.2/1.2 = 1
Hydrogen	1.2	1	1.2/1 = 1.2	1.2/1.2 = 1
Chlorine	84.5	35.5	84.5/35.5 = 2.38	2.38/1.2 = 2

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,Cl=35.5]

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