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Mole Concept Basic - Practice Questions & MCQ
Edited By admin | Updated on Sep 18, 2023 18:34 AM | #JEE Main
Quick Facts
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MOLE CONCEPT AND MOLAR MASS is considered one the most difficult concept.
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77 Questions around this concept.
Solve by difficulty
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
The number of water molecules is maximum in :
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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The number of molecules and moles in 2.8375 litres of at STP are respectively
Match List I with List II
Choose the correct answer from the options given below:
A sample of $\mathrm{CaCO}_3$ and $\mathrm{MgCO}_3$ weighed $2.21 \mathrm{~g}$ is ignited to constant weight of $1.152 \mathrm{~g}$. The composition of mixture is: (Given molar mass in $\mathrm{g} \mathrm{mol}^{-1} \mathrm{CaCO}_3: 100, \mathrm{MgCO}_3: 84$ )
Molar Mass = Vapour density X 2 , is valid for :
How many atoms are contained in a mole of 2- HYDROXY-PROPANOIC ACID (Lactic acid).
How many volume will $\mathrm{CO}_2$ gas will occur in 88 g of its at STP?
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Try NowNumber of moles in 80 g of Calcium is
Concepts Covered - 1
MOLE CONCEPT AND MOLAR MASS
Mole:
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A mole is a unit that represents 6.023 x 1023 particles, atoms, molecules or ions, etc., irrespective of their nature.
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Mole is related to the mass of the substance, the volume of gaseous substance and the number of particles
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Here G.m.m. = Gram molecular mass or molar mass which is the mass of 1 mole of any substance
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The volume of one mole of any gas is equal to 22.4 litres or dm3 at STP. It is known as molar volume.
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Relationship of Mole:
A mole of any substance (like O2) stands for:
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6.023 x 1023 molecules of O2
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2 x 6.023 x 1023 atoms of Oxygen
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32 gm of Oxygen
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22.4 litre of O2 at STP.
To Find the Total Number of Identities:
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Total number of Molecule = mole(n) x NA
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Total number of Atoms = mole (n) x NA x No. of atoms present in one molecule (atomicity).
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Total number of Electrons = mole (n) x NA x No. of electron present in one atom.
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Total charge on any ion = mole (n) x NA x charge on one ion x 1.6 x 10-19 C
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