how may minutes it take to plate out 5.0 g of Cr from cr2(So4)3 solution using a current of 1.50 A? (At. Weight ; Cr = 52)
Current = 1.50 A
Cr3+ + 3e- Cr
Molar mass of Cr = 52 g/mol
Thus 1 mole = 52 g Cr is deposited by 3 F (289500 C ).
Therefore 5.0 g Cr will be deposited by = C = 27836.54 C
Now Q= I t
where Q is charge
I is current = 1.50 A
t is time
Thus t = = 18557.69 seconds
= 309.29 minutes
Cr3+ + 3e- Cr
Molar mass of Cr = 52 g/mol
Thus 1 mole = 52 g Cr is deposited by 3 F (289500 C ).
Therefore 5.0 g Cr will be deposited by = C = 27836.54 C
Now Q= I t
where Q is charge
I is current = 1.50 A
t is time
Thus t = = 18557.69 seconds
= 309.29 minutes