Question

Which has the maximum number of atoms?
(A) $ 24{{ }}g{{ }}of{{ }}C{{ }}\left( {12} \right) $
(B) $ 56{{ }}g{{ }}of{{ }}Fe{{ }}\left( {56} \right) $
(C) $ 27{{ }}g{{ }}of{{ }}Al{{ }}\left( {27} \right) $
(D) $ 108{{ }}g{{ }}of{{ }}Ag{{ }}\left( {108} \right) $

Answer 1

Hint: The mole idea is an advantageous strategy for communicating the measure of a substance. Any estimation can be separated into two sections – the mathematical extent and the units that the greatness is communicated in.

Complete Step By Step Solution:
In the field of science, a mole is characterized as the measure of a substance that contains precisely $ 6.02214076{{ }} \times {{ }}{10^{23}} $ 'rudimentary elements' of the given substance. The number $ 6.02214076{{ }} \times {{ }}{10^{23}} $ is prevalently known as the Avogadro steady and is frequently meant by the image ' $ {N_A} $ '. The rudimentary elements that can be spoken to in moles can be iotas, atoms, monatomic/polyatomic particles, and different particles, (for example, electrons).
For instance, one mole of an unadulterated carbon-12 $ \left( {12C} \right) $ example will have a mass of precisely 12 grams and will contain $ 6.02214076{{ }} \times {{ }}{10^{23}} $ $ \left( {NA} \right) $ number of $ 12C $ molecules. The quantity of moles of a substance in a given unadulterated example can be spoken to by the accompanying recipe:
 $ n{{ }} = {{ }}\frac{N}{{{N_A}}} $
Where $ n $ is the quantity of moles of the substance (or rudimentary element), $ N $ is the complete number of rudimentary elements in the example, and $ {N_A} $ is the Avogadro constant.
 $ 12{{ }}g $ of $ C $ contains $ {N_A} $ various molecules. Accordingly, $ 24{{ }}g $ of $ C $ contains 2 $ {N_A} $ number of iotas. Likewise, $ {{56 }}g $ of $ Fe $ , $ 27{{ }}g $ of $ Al $ and $ 108{{ }}g $ of $ Ag $ contain $ {N_A} $ number of molecules. Accordingly, the greatest number of particles is available in $ 24g $ of $ C $ .
Option A is correct.

Additional Information:
"Mole" was presented around the year 1896 by the German scientist Wilhelm Ostwald, who got the term from the Latin word moles meaning a 'pile' or 'heap. The nuclear mass of a component is the mass of one particle of the component communicated in nuclear mass units (amu). It represents the bounty of the different isotopes of the component and doles out a normal incentive to the mass of one iota of the component.
The molar mass of a substance is characterized as the all out mass of one mole of the substance. It is regularly spoken to as far as 'grams per mole' . In any case, the SI unit of this amount is $ kg/mol $ . Molar mass can be spoken to by the accompanying recipe:
 $ Molar{{ }}mass{{ }}of{{ }}a{{ }}Substance{{ }} = \frac{{{{ }}\left( {Mass{{ }}of{{ }}the{{ }}Substance{{ }}in{{ }}grams} \right)}}{{\left( {Number{{ }}of{{ }}Moles} \right)}} $

Note:
When managing particles at a nuclear (or sub-atomic) level, even one gram of an unadulterated component is known to contain countless molecules. This is the place where the mole idea is broadly utilized. It principally centers around the unit known as a 'mole', which is a tally of countless particles.