Respuesta :
Answer :
(a) The number of atoms of nickel required are, [tex]5.988\times 10^{23}[/tex]
(b) The moles of nickel are, and 0.9944 mol
Explanation : Given,
Area = [tex]200in^2=200\times 6.45=1290cm^2[/tex]
Conversion used : [tex](1in^2=6.45cm^2)[/tex]
Thickness = 0.002 in = 0.002 × 2.54 = 0.00508 cm
Conversion used : (1 in = 2.54 cm)
First we have to calculate the volume of nickel.
Volume of nickel = Area × Thickness
Volume of nickel = [tex]1290cm^2\times 0.00508cm[/tex]
Volume of nickel = [tex]6.55cm^3[/tex]
Now we have to calculate the mass of nickel.
Mass of nickel = Density of nickel × Volume of nickel
Density of nickel = 8.91 g/cm³
Mass of nickel = 8.91 g/cm³ × 6.55 cm³
Mass of nickel = 58.36 g
Now we have to calculate the moles of nickel.
[tex]\text{Moles of nickel}=\frac{\text{Mass of nickel}}{\text{Molar mass of nickel}}[/tex]
Molar mass of nickel = 58.69 g/mol
[tex]\text{Moles of nickel}=\frac{58.36g}{58.69g/mol}=0.9944mol[/tex]
Now we have to calculate the number of atoms of nickel are required.
As, 1 mole of nickel contains [tex]6.022\times 10^{23}[/tex] atoms of nickel
So, 0.9944 mole of nickel contains [tex]0.9944\times 6.022\times 10^{23}=5.988\times 10^{23}[/tex] atoms of nickel
Thus, the number of atoms of nickel required and moles of nickel are, [tex]5.988\times 10^{23}[/tex] and 0.9944 mol respectively.
