Answer:
[tex]0.168631 \ moles \ Al[/tex]
Explanation:
Atomic mass of [tex]Al[/tex] is given as [tex]26.982u[/tex], where [tex]u[/tex] is the unified atomic mass unit.
[tex]u[/tex] is defined as [tex]\frac{1}{12}[/tex]th the mass of a neutral carbon-12 atom. This is equal to the mass of [tex]one \ nucleon[/tex]. Therefore:-
[tex]1u=1g/mol\\[/tex]
Mole constant=[tex]6.022\times10^{23}[/tex] atoms of any element.
For [tex]Al[/tex] of 12g:-
[tex]12\times \frac{1 \ mole \ Al}{26.982g}\\=0.168631 \ moles[/tex][tex]=12\times\frac{1 \ mole \ Al}{26.982g}\\=0.168631 \ moles \ Al[/tex]
There are 0.168 moles of atoms in the 12 g of Aluminium. A mole is a constant number of atoms, ions, and particles.
A mole is a constant number of atoms, ions, and particles which is equal to Avogadro's constant.
1 mole = [tex]6.02 \times 10^2^3[/tex]
The formula of the mole is,
[tex]n = \dfrac wm[/tex]
Where,
[tex]n[/tex] - number of moles
[tex]w[/tex] - given mass = 12 g
[tex]m[/tex] - molar mass = 26.98 g/mole
Put the values in the formula,
[tex]n = \dfrac{12}{27.98}\\\\n = 0.168 \rm \ mole[/tex]
Therefore, there are 0.168 moles of atoms in the 12 g of Aluminium.
Learn more about the Mole concept:
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