Answer: 8.95 hours
Explanation:
[tex]Ni^{2+}+2e^-\rightarrow Ni[/tex]
[tex]96500\times 2=193000[/tex] Coloumb of electricity deposits 1 mole of Nickel
1 mole of Nickel weighs = 58.7 g
Given quantity = 1.0 kg = 1000 g (1kg=1000g)
58.7 g of Nickel is deposited by 193000 C of electricity
1000 g of Nickel is deposited by =[tex]\frac{193000}{58.7}\times 1000=3287904.6C[/tex] of electricity
[tex]Q=I\times t[/tex]
where Q= quantity of electricity in coloumbs = 3287904.6C
I = current in amperes = 102 A
t= time in seconds = ?
[tex]3287904.6C=102A\times t[/tex]
[tex]t=32234.359sec[/tex]
[tex]t=8.95hr[/tex] (1h=3600 sec)
Thus 8.95 hours it takes to plate out 1.0 kg Ni from aqueous [tex]Ni^{2+}[/tex] solution, if the electrical current is 102 A.
It will take 8.95 hours to plate out 1.0 kg Ni from aqueous
[tex]Ni^{2+}[/tex]
solution, if the electrical current is 102 A.
Electroplating is the process of covering the surface of a metal with another metal through the process of electrolysis.
The equation of the reaction is given as follows:
[tex]Ni^{2+}+2e^
→Ni[/tex]
From the equation of the reaction, 2 moles of electrons = 2 × 96500 C of electricity are required to deposit 1 mole or 58.7 g of Nickel
1..0 kg of nickel = 1000 g
58.7 g of Nickel is deposited by 193000 C of electricity
1000 g of Nickel is deposited by 1000 × 193000/58.7 =3287904.6C of electricity
The time take required is calculated from the formula:
Quantity of charge, Q = current, I × time
Time = Q/I
Time = =3287904.6/102
Time = 32234.359 seconds
Converting time to hours; 1 hour =3600 seconds
Time =32234.359/3600
Time = 8.95 hours
Therefore, if the current is 102 A, 8.95 hours required to plate out 1.0 kg Ni from aqueous Nickel (ii) ion.
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