Answer: [tex]2.2326\times 10^{-3}[/tex] moles
Explanation:
We are given:
Moles of electron = 1 mole
According to mole concept:
1 mole of an atom contains [tex]6.022\times 10^{23}[/tex] number of particles.
We know that:
Charge on 1 electron = [tex]1.6\times 10^{-19}C[/tex]
Charge on 1 mole of electrons = [tex]1.6\times 10^{-19}\times 6.022\times 10^{23}=96500C[/tex]
The metal being plated has a +4 charge, thus the equation will be:
[tex]M^{4+}+4e^-\rightarrow M[/tex]
[tex]4\times 96500C[/tex] of electricity deposits = 1 mole of metal
Thus 861.8 C of electricity deposits =[tex]\frac{1}{4\times 96500}\times 861.8=2.2326\times 10^{-3}[/tex] moles of metal
Thus [tex]2.2326\times 10^{-3}[/tex] moles of metal should be plated
The number of moles of the metal deposited is 0.0022 moles of metal.
The term electroplating refers to the use of one metal to cover the surface of another metal. Let the metal in question be M, the equation of the reaction is; M^4+(aq) + 4e -----> M(s).
1 mole of the metal is deposited by 4( 96,500) C
x moles will be deposited by 861.8 C
x = 1 mole * 861.8 C/ 4( 96,500) C
x = 0.0022 moles of metal
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