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    Mole Concept Basic MCQ - Practice Questions with Answers

    Edited By admin | Updated on Sep 25, 2023 25:23 PM | #NEET

    Quick Facts

    • MOLE CONCEPT AND MOLAR MASS is considered one the most difficult concept.

    • 47 Questions around this concept.

    Solve by difficulty

    QuestionEASY

    If we consider that 1/6, in place of 1/12, mass of carbon atom is taken to be the relative atomic mass unit, the mass of one mole of a substance will

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    The number of water molecules is maximum in :

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    Which has the maximum number of molecules among the following?

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    Which one of the following has a maximum number of atoms?

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    If Avogadro number NA, is changed from 6.022 x 1023 mol-1 to 6.022 x 1020 mol-1, this would change :

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    A mixture of gases contains H2 and O2 gases in the ratio of 1 : 4 (w/w). What is the molar ratio of the two gases in the mixture ?

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    The volume of oxygen at STP Requires to burn  0.8 g of carbon completely is?

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    Concepts Covered - 1

    MOLE CONCEPT AND MOLAR MASS

    Mole:

    • A mole is a unit that represents 6.023 x 1023 particles, atoms, molecules or ions, etc., irrespective of their nature.

    • Mole is related to the mass of the substance, the volume of gaseous substance and the number of particles

    • \mathrm{Mole = \frac{W}{M} = \frac{\textrm{(Wt. of substance in gm.) }}{(\textrm{Molar mass of substance (G.m.m)})}}

    Here G.m.m. = Gram molecular mass

    • \mathrm{Mole = \frac{(\textrm{Volume of substance in litre}) }{22.4\ litre}}

    • Volume of one mole of any gas is equal to 22.4 litres of dm3 at STP. It is known as molar volume.

    • \mathrm{Mole = \frac{\textrm{Number of identities}}{\textrm{Avogadro's number}}}

    • \mathrm{Mole =\frac{ PV }{RT }}

    Here P= Pressure in atmosphere, V = Volume in litre, T = Temperature in Kelvin, R = Universal gas constant

     

     

    Relationship of Mole:

     A mole of any substance (like O2) stands for: 

    • 6.023 x 1023  molecules of O2 

    • 2 x 6.023 x 1023 atoms of Oxygen 

    • 32 gm of Oxygen

    • 22.4 litre of O2 at STP.

     

    To Find the Total Number of Identities:

    1. Total number of Molecule = mole(n) x NA

    2. Total number of Atoms = mole (n) x NA x No. of atoms present in one molecule 

    3. Total number of Electrons = mole (n) x NA  x No. of electron present in one electron

    4. Total charge on any ion = mole (n) x NA x charge on one ion x 1.6 x 10-19 C

     

    Determination of Molar mass:

    1. Vapour Density method -

    1. Vapour Density of gas is defined as the ratio of the weight of  certain volume of a gas to the weight of the same volume of hydrogen at the same temperature and pressure 

    \mathrm{\textrm{Vapour density of a gas} = \frac{\textrm{weight of V litres of the gas}}{\textrm{Weight of V litres of } H_2 \textrm{ at the same temperature and pressure}}}

     

    1. \mathrm{Vapour\ Density = (Molecular\ mass) / 2 }

    1. Graham Diffusion Method - 

    \mathrm{r_1 / r_2 = (M_2/M_1)^{1/2} }

    Here r1 ,  r2 are rates of diffusion for two species while M1, M2 are their molecular masses respectively. 

    1. Colligative Properties -

    \pi V=\frac{W}{m}RT

    Here, \mathrm{\pi = \textrm{Osmotic pressure in atm}}

    V = Volume in litre

    W = Weight in grams 

    R = Universal gas Constant

    T = Given Temperature

    m = Molar mass

    Study it with Videos

    MOLE CONCEPT AND MOLAR MASS

    Study other Related Concepts

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    Mole Concept Basic
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    Empirical and Molecular Formula
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    Books

    Reference Books

    MOLE CONCEPT AND MOLAR MASS

    Chemistry Part I Textbook for Class XI

    Page No. : 18

    Line : 5

    Clear your Basics with NCERT

    E-books & Sample Papers

    NEET Mock Test Botany (Biology) 2027

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