Question

How many minutes will it take to plate out 5.2 g of Cr from a Cr2(SO4)3 solution usine
current of 9.65 A? (Atomic weight : Cr = 52.0)
(a) 200
(b) 50 g
(c) 100
(d) 103

solution k sath (+_+)​

Answer 1

ANSWER:

Current = 1.50 A

${Cr}^{3 + } + \: ( {3}^{e - } ) \: → \: Cr$

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 =

$\frac{289500}{52} \times 5 C = 27836.54 C$

Now Q= I× t

where Q is charge

I is current = 1.50 A

t is time

$Thus \: \: \: t = \frac{27836.54}{1.5} = \: 18557.69 \: seconds$

= 309.29 minutes

Answer 2

$\huge\sf\underline{♡Answer♡}$

Current = 1.50 A

${Cr}^{3 + } + \: ( {3}^{e - } ) \: → \: Cr$

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 =

$\frac{289500}{52} \times 5 C = 27836.54 C$

Now Q= I× t

where Q is charge

I is current = 1.50 A

t is time

$Thus \: \: \: t = \frac{27836.54}{1.5} = \: 18557.69 \: seconds$

= 309.29 minutes