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A compound contains three elements carbon, hydrogen and nitrogen in the respective ratio of $9 : 1 : 3.5$ by mass. The empirical formula for the compound will not be:

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Important Questions on Some Basic Concepts of Chemistry

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

An organic compound contains

24 %

carbon,

4 %

hydrogen and remaining chlorine. Its empirical formula is

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

The ratio of mass percent of

C and H

of an organic compound

(C_{X} H_{Y} O_{Z})

6 : 1 .

If one molecule of the above compound

(C_{X} H_{Y} O_{Z})

contains half as much oxygen as required to burn one molecule of compound

C_{X} H_{Y}

completely to

{CO}_{2}

and

H_{2} O .

The empirical formula of the compound

C_{X} H_{Y} O_{Z}

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

The percentage composition of carbon by mole in methane is:

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

In Carius method of estimation of halogens,

250 mg

of an organic compound gave

141 mg AgBr

. What is the percentage of bromine in the compound (atomic mass of

Ag = 108

and atomic number of

Br = 80

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

A compound has the following composition by weight;

N a = 18.60 %, S = 25.80 %, H = 4.02 %

and

O = 51.58 %

Assuming that all the hydrogen atoms in the compound are part of water of crystallization, the correct molecular formula of the compound is

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

In an estimation of bromine by Carius method,

1.6 g

of an organic compound gave

1.88 g

AgBr

. The mass percentage of bromine in the compound is

\dots . .

(

Atomic mass,

Ag = 108, Br = 80 {gmol}^{- 1}

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

An organic compound contains

C, H

and

S

. The minimum molecular weight of the compound containing

8 %

Sulphur is

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

A metal

M

(specific heat

0.16

) forms a metal chloride with

65 %

chlorine present in it. The formula of the metal chloride will be

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

1.25 g of a metal (M) reacts with oxygen completely to produce 1.68 g of metal oxide. The empirical formula of the metal oxide is [Molar mass of M and O are

69.7 g m o l^{- 1}

and

16.0 g m o l^{- 1}

, respectively]

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

1.85 g

sample of an arsenic-containing pesticide was chemically converted to

{AsO}_{4}^{3 -}

(atomic mass of

As = 74.9

) and titrated with

{Pb}^{2 +}

to form

{Pb}_{3} {({AsO}_{4})}_{2}

. If

20 mL of 0.1 M {Pb}^{2 +}

is required to reach the equivalence point, the mass percentages of arsenic in the pesticide sample is closest to

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

The empirical formula and molecular mass of a compound are

{CH}_{2} O

and

180 g

respectively. The molecular formula of the compound will be

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

Mass % of carbon in ethanol is

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

Calculate the percentage by weight of oxygen in a mole of water?

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

Complex A has a composition of

H_{12} O_{6} {Cl}_{3} C r

. If the complex on treatment with conc.

H_{2} {SO}_{4}

loses

13.5 %

of its original mass, the correct molecular formulas of

A

is:
[Given : atomic mass of

C r = 52

amu and

Cl = 35

amu]

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

1 g

of an organic compound containing

C

and

H

, on complete combustion produced

3.04 g

{CO}_{2}

and

1.53 g

H_{2} O

. Find the approximate percentage composition of

C

and

H

in the compound.

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

Complete combustion of

750 g

of an organic compound provides

420 g

{CO}_{2}

and

210 g

H_{2} O

. The percentage composition of carbon and hydrogen in organic compound is

15.3

and ______ respectively. (Round off to the Nearest Integer)

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

In the crystalline solid

M S O_{4} \cdot n {II}_{2} O

of molar mass

250 g {mol}^{- 1},

the percentage of anhydrous salt is

64

by weight. The value of

n

HARD

Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

One mole of one of the sodium salts listed below, having carbon content close to

14.3 %

produces

1

mole of carbon dioxide upon heating

(Atomic masses : Na = 23, H = 1, C = 12, O = 16)

. The salt is

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

The percentage of nitrogen by mass in ammonium sulphate is closest to (atomic masses H = 1, N = 14, O = 16, S = 32)

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Chemistry>Physical Chemistry>Some Basic Concepts of Chemistry>Empirical and Molecular Formulae

A sample of a hydrate of barium chloride weighing 61 g was heated until all the water of hydration is removed. The dried sample weighed 52 g. The formula of the hydrated salt is: (atomic mass, Ba = 137 amu, Cl = 35.5 amu)

A compound contains three elements carbon, hydrogen and nitrogen in the respective ratio of 9:1:3.5 by mass. The empirical formula for the compound will not be:

Important Questions on Some Basic Concepts of Chemistry

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A compound contains three elements carbon, hydrogen and nitrogen in the respective ratio of $9 : 1 : 3.5$ by mass. The empirical formula for the compound will not be: