ECAT Pre Engineering Chemistry Chapter 1 MCQ Test With Answer

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ECAT Chemistry Chapter 1 Important MCQ's

Sr.#	Question	Answer
1	The value of R(General Gas Constant) is	A. 8.3134 JK^-1mole^-1 B. 1.987 Cal K^-1Mole^-1 C. Both a and b D. 1.987 JK^-1mole^-1
2	A beaker contains 9 grams of water. The number of H-atoms is	A. 6.02 x 1023 B. 3.01 x 1023 C. 6.02 x 1024 D. 3.01 x 1024
3	A compound contains 75% carbon and 25% hydrogen, by mass. What is the molecular formula of the compound/	A. C₃H₈ B. CH₄ C. C₂H₄ D. C₂H₆
4	The negatively charged particles are called	A. Cation B. Radical C. Anion D. Positron
5	The volume occupied by 1.4 g of N₂at S.T.P is	A. 2.24 dm³ B. 22.4 dm³ C. 1.12 dm³ D. 112 cm³
6	NH₃, HCL, H₂O, HL are:	A. Diatomic molecules B. Poly-atomic molecules C. Mono-atomic molecules D. Hetero atomic molecules
7	Which has greater number of moles	A. 0.1 g sodium B. 6.02 x 10²⁰atoms of magnesium C. 20 cm³0.1mole per dm³of NaOH D. 12.2 dm³of nitrogen at standard [A_rNa = 23, Mg = 24, O = 16]
8	Formation of a cation is:	A. Exothermic process B. Non-endothermic process C. Endothermic process D. None of above
9	The isotopes of an element	A. Possess same mass number B. Possess same number of protons C. Do not possess same chemical properties D. May or may not possess same chemical properties
10	What is the maximum mass of aluminium which can be obtained from 240g of aluminium oxide Al₂O₃?	A. 26 g B. 127 g C. 51 g D. 108 g

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ECAT Pre Engineering Chemistry Chapter 1 MCQ Test With Answer

MCQ's Test For ECAT Chemistry Chapter 1 Basic Concepts

ECAT Chemistry Chapter 1 Basic Concepts

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

Isotopes of an element differ in

The pressure of vapours when sent to the ionization chamber in mass spectrometer is

Ascorbic acid contains 40.92% carbon, 4.58%, hydrogen and 54.4% oxygen. The empirical formula is

3.01 x 1022Ag+ions is present in

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

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

Which of the sub-atomic particles is not charged

Hemoglobin contains nearly:

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

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

One mole of SO2contains

Which statement about molecule is incorrect ?

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

0.5 mole of CH4and 0.5 mole of SO2gases have equal

The atom of an element is

The percentage of H is the highest in

The isotopes of an element

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

C6H12O6and C12H22O11 are:

The largest number of molecules are present in

Atoms can be evident by use of electron microscope, field ionization microscope and:

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

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

A species having positive or negative charge is called:

A limiting reactant is the one which

The mass of Al2S3formed when 20 grams Al reacts completely with S is

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

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

The number of atoms present in molecule determines its:

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ECAT Chemistry Chapter 1 Important MCQ's

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

3.01 x 10²²Ag⁺ions is present in

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

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

One mole of SO₂contains

0.5 mole of CH₄and 0.5 mole of SO₂gases have equal

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

C₆H₁₂O₆and C₁₂H₂₂O₁₁ are:

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

The mass of Al₂S₃formed when 20 grams Al reacts completely with S is