When 3.86 amperes current is passes through an electrolyte for 50 minutes, 2.4 grams of a divalent metal is deposited. The gram atomic weight of the metal (in grams) is :

Q. A solution of metal salt was electrolyzed for

15

minutes, with a current of

1.5 A

. The mass of a metal deposited was

0.00783 k g

. Calculate the equivalent mass of metal.

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How many grams of cobalt metal will be deposited when a solution of cobalt(II) chloride is electrolyzed with a current of 10 amperes for 109 minutes? (1 Faraday=96,500 C;Atomic mass of Co = 59 u)

The correct option is B 20.0We know that, w=IEt96500 w=10×109×60×5996500×2 =19.99≈20 g

How many grams of cobalt metal will be deposited when a solution of cobalt(II) chloride is electrolyzed with a current of $10$ amperes for $109$ minutes? $(1 Faraday = 96, 500 C; Atomic mass of Co = 59 u)$

The correct option is B $20.0$
We know that,
$w = \frac{I E t}{96500}$
$w = \frac{10 \times 109 \times 60 \times 59}{96500 \times 2}$
$= 19.99 \approx 20 g$