A solution of is electrolyzed for '' min with a current of 1.5 A to deposit 0.3482 g of Fe. The value of x is [nearest integer]

Given: . Atomic mass of

Question

A solution of  is electrolyzed for '' min with a current of 1.5 A to deposit 0.3482 g of Fe. The value of x is  [nearest integer]

Given: . Atomic mass of

Canvas Classes · Accepted Answer

Strategy:
 Use Faraday's Law to relate the mass of deposited metal to the current and time. Be careful with the valence () of the metal ion in the specific salt.

Step 1: Calculate moles of Iron
Mass deposited . Atomic mass .

Step 2: Relate to Faradays
From , Iron is in the  state ().
Reductions: .
Total charge .

Step 3: Calculate time
.

More questions from Electrochemistry