Question # 1

Which of the sub-atomic particles is not charged

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Electron

Proton

Neutron

All of them

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

What is the maximum mass of aluminium which can be obtained from 240g of aluminium oxide Al₂O₃?

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26 g

127 g

51 g

108 g

A compound having empirical formula C₃H₃O and its molecular mass is 110.02. Its molecular formula is

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C₃H₃O

C₆H₆O₂

C₉H₉O₃

C₃H₆O₂

A beaker contains 9 grams of water. The number of H atoms is

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6.02 x 10²³

3.01 x 10²³

6.02 x 10²⁴

3.01 x 10²⁴

A species having positive or negative charge is called:

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Electron

Ion

Proton

Atom

The quantitative relationship between the substances according to balanced equation describes

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Reversible reactions

Stoichiometry

Limiting reacting

Percentage composition

Relative atomic mass of an element is the mass of the element relative to

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1/12 mass of carbon-12

1/12 mass of carbon

1 mass of hydrogen atom

1/16 mass of oxygen

The volume occupied by 1.4 g of N₂at S.T.P is

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2.24 dm³

22.4 dm³

1.12 dm³

112 cm³

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

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Positrons

Photons

Ions

Electrons

Which of the following statement is correct for a chemical reaction to occur molecules of substances must

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Collide with each other

Collide with energy more than activation energy

Collide with energy less than activation energy

Collide with high frequency

CL₂, N₂ and O_{2 are:}

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Diatomic molecules

Hetero atomic molecules

Poly-atomic molecules

Mono-atomic molecules

A compound X contains 50% sulphur and 50% oxygen by mass. What is the empirical formula of compound X?

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SO

SO₂

SO₃

SO₄

Mass spectrometer measures the

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Exact mass of an element

Average mass of an element

The number of elements present in a molecule

m/e value of a positive ion

How many moles of hydrogen atoms does 3.2 g of methane, CH₄, contain?

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0.02

0.2

0.4

0.8

Metal tend to lose electrons, becoming:

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Metals

Positively charged

Negatively charged

(a)And (c)

A molecular ion is formed by

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Passing a high energy electron beam through gaseous molecule

Dissolving a salt i dilute acid

Passing electric current through molten salt

Passing electricity through aqueous solutions

Which one of the following step is not involved in determination of empirical formula

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Determination % of each element

Determination of gram atom of each element

Determination of isotopes of each element

Determination of atomic ratio of element

The relative abundance of Pb isotopes is 1.5% Pb²⁰⁴, 23.6% Pb²⁰⁶, 22.6% Pb²⁰⁷, 52.3% Pb²⁰⁸The relative atomic mass of Pb is

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207.94

208.24

206.94

207.24

0.5 mole of CH4and 0.5 mole of SO2gases have equal

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Volume

Mass in grams

Total number of atoms

Number of molecules

The value of R(General Gas Constant) is

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8.3134 JK^-1mole^-1

1.987 Cal K^-1Mole^-1

Both a and b

1.987 JK^-1mole^-1

1.12 dm³of N₂gas at S.T.P. has mass of N₂gas

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2.8 g

2.4 g

1.4 g

14 g

A beaker contains 9 grams of water. The number of H-atoms is

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6.02 x 1023

3.01 x 1023

6.02 x 1024

3.01 x 1024

A molecule of haemoglobin is made up if nearly

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10,000 atoms

50,000 atoms

2500 atoms

1500 atoms

Which statement about an atom is true ?

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The number of neutrons is not equal to number of electrons

Mass number is less than atomic number

All the elements have only one mass number

Mass number can be equal to atomic number

3.01 x 10²²Ag⁺ions is present in

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85 grams AgNO₃

0.85 g AgNO₃

8.5 g AgNO₃

18.5 g AgNO₃

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

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

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300 cm³

200 cm³

150 cm³

100 cm³

C₆H₁₂O₆and C₁₂H₂₂O₁₁ are:

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Mono-atomic molecules

Diatomic molecules

Poly-atomic molecules

Hetero atomic molecules

He Ar and Ne are:

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Mono-atomic molecules

Hetero atomic molecules

Poly-atomic molecules

Diatomic molecules

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