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) :

Question

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) : (A) 4.0 (B) 20.0 (C) 40.0 (D) 0.66

Tardigrade Admin · Accepted Answer

W =(I t E/96500) =(10 × 109 × 60 × 59/96500 × 2) =19.99 ≈ 20

Q. 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) :

4.0

20.0

40.0

0.66

$W = \frac{I tE}{96500}$
$= \frac{10 \times 109 \times 60 \times 59}{96500 \times 2}$
$= 19.99 \approx 20$

Q. 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) :

4.0

20.0

40.0

0.66

W=96500ItE​ =96500×210×109×60×59​ =19.99≈20

$W = \frac{I tE}{96500}$
$= \frac{10 \times 109 \times 60 \times 59}{96500 \times 2}$
$= 19.99 \approx 20$