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
‚ÄčMolar mass of Cr = 52 g/mol
Thus 1 mole = 52 g Cr is deposited by 3 F (289500 C ).
‚ÄčTherefore 5.0 g Cr will be deposited by = 28950052×5 C = 27836.54 C

Now Q= I× t
where Q is charge
I is current = 1.50 A
t is time

Thus t = 
27836.541.5 = 18557.69 seconds

                            = 309.29  minutes

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