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MOLE CONCEPT AND MOLAR MASS is considered one the most difficult concept.
29 Questions around this concept.
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
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 $\mathrm{g} \mathrm{mol}^{-1} \mathrm{CaCO}_3: 100, \mathrm{MgCO}_3: 84$ )
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
Here G.m.m. = Gram molecular mass or molar mass which is the mass of 1 mole of any substance
The volume of one mole of any gas is equal to 22.4 litres or dm3 at STP. It is known as molar volume.
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:
Total number of Molecule = mole(n) x NA
Total number of Atoms = mole (n) x NA x No. of atoms present in one molecule (atomicity).
Total number of Electrons = mole (n) x NA x No. of electron present in one atom.
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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