Question # 1

Matter is defined as any thing which occupies space and:

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Molecules

Mass

Compound

Molecules

Which of the following compounds contains the highest percentage by mass of nitrogen?

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Ammonia, NH₃

Ammonium carbamate, NH₂CO₂NH₄

Ammonium carbonate, (NH₄)₂CO₃

Hydrazine, N₂H₄

CL₂, N₂ and O_{2 are:}

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Diatomic molecules

Hetero atomic molecules

Poly-atomic molecules

Mono-atomic molecules

Objects of the size of an atom can be observed in

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An electron microscope

An x-ray spectrum

Atomic absorption spectrum

A visible spectrum

Which of the following statements is not true?

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Isotopes with even atomic masses are comparatively abundant

Isotopes with even atomic masses and even atomic numbers are comparatively abundant

Isotopes with even atomic masses and odd atomic number are comparatively abundant

A species having positive or negative charge is called:

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Electron

Ion

Proton

Atom

The amount of products obtained from the balanced chemical equation is regarded as

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Theoretical yield

Actual yield

% yield

Experimental yield

The atom of an element is

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The smallest particle

The fundamental particle

The independent particle

The charged particle

Covalent compound s mostly exist in the form of:

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Protons

Atoms

Neutrons

Molecules

How many moles of oxygen, O₂are needed for the complete combustion of two moles of butane C₄H₁₀?

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2

8

10

13

Benzene is stable to:

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Oxidation

Nitration

KMnO₄

SULPHONATION

Who one mole of each of the following is completely burned in oxygen, which gives the largest mass of carbon dioxide?

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Carbon monoxide

Diamond

Ethane

Methane

What is the volume in cm³of 3.01 x 10²³molecules of O₂gas at S.T.P

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1000 cm³

11000 cm³

1120 cm³

11200 cm³

C₆H₁₂O₆and C₁₂H₂₂O₁₁ are:

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Mono-atomic molecules

Diatomic molecules

Poly-atomic molecules

Hetero atomic molecules

When nitrogen is 5.6 grams in NO₂. then number of moles of NO₂is

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0.5

0.4

0.04

0.05

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84.84 %

89.89%

81.81%

90.90%

Determination of atomic masses and invention of system of writing symbols was made by:

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J. Berzelius

Democritus

Dalton

None of above

When 0.1 g of magnesium is treated with an excess of hydrochloric acid, what volume of gas at room temperature and pressure will be produced

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10 cm³

25 cm³

48 cm³

100 cm³

Atoms and molecules can either gain or lose electrons, forming charge particles called:

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Positrons

Photons

Ions

Electrons

The atomic mass is measured in atomic mass unit (a.m.u.) which is equal to

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1.661 x 10^{-27- Kg}

1.661 x 10^-24Kg

1.661 x 10^{-27- g}

1.661 x 10^-24mg

The negatively charged particles are called

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Cation

Radical

Anion

Positron

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N₂O₄is limiting reactant

N₂H₄is the limiting reactant

Reactants are completely converted to the products

Reactions is reversible

The branch of science dealing with structure, composition and changes in matter and laws and principles which govern these changes is called as

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chesmistry

Geology

Physics

Mechanics

Each molecule of haemoglobin is 68000 times heavier than one atom of

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C

H

N

O

The relative atomic mass of chlorine is 35.5. What is the mass of 2 mol of chlorine gas

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142 g

71 g

35.5 g

18.75 g

NH₃, HCL, H₂O, HL are:

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Diatomic molecules

Poly-atomic molecules

Mono-atomic molecules

Hetero atomic molecules

The isotopes of an element

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Possess same mass number

Possess same number of protons

Do not possess same chemical properties

May or may not possess same chemical properties

One mole of C₂H₅OH contains the number of H-atoms

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6.02 x 10²³

3.61 x 10²⁴

1.81 x 10²⁴

6.02 x 10²⁴

The empirical formula of a liquid compound is known to be C₂H₄O. What other information is needed to work out its molecular formula?

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The percentage composition of the compound

The relative molecular mass of the compound

The density of the compound

The volume occupied by one mole of the compound

Two different hydrocarbon each contain the same percentage by mass of hydrogen. It follows that they have the same

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Empirical formula

Number of atoms in a molecules

Number of isomers

Relative molecular mass

Isotopes differ in

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properties which depend upon mass

arrangement of electrons in orbitals

chemical properties

the extent to which they may be affected in electric fields

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