Answer: 4.6 grams
Explanation:
1 electron carry charge=[tex]1.6\times 10^{-19}C[/tex]
1 mole of electrons contain=[tex]6.023\times 10^{23}[/tex] electrons
Thus 1 mole of electrons carry charge=[tex]\frac{1.6\times 10^{-19}}{1}\times 6.023\times 10^{23}=96500C[/tex]
[tex]A^{n+}\rightarrow A+ne^-[/tex]
[tex]Q=I\times t[/tex]
where Q= quantity of electricity in coloumbs
I = current in amperes = 0.800A
t= time in seconds = 100 min= 6000 sec (1min=60sec)
[tex]Q=0.800A\times 6000s=4800C[/tex]
96500C charge is carried by = 1 mole of electrons
4800C charge is carried by= [tex]\frac{1}{96500}\times 4800=0.05moles[/tex]
[tex]Mass={\text {no of moles}}\times {\text {Molar mass}}=0.05moles\times 92.708g/mol=4.6g[/tex]
Thus 4.6g of [tex]Ni(OH)_2[/tex] is oxidized to [tex]NiO(OH)[/tex].
