0.2 Faraday Charge is passed in 1litre solution containing 0.1molar fe3+ions how many moles of iron get deposited at cathode assuming only iron is reduced to electrolitic process

To determine how many moles of iron get deposited at the cathode when 0.2 Faraday of charge is passed through a 1-liter solution containing 0.1 molar Fe³⁺ ions, we can use Faraday's laws of electrolysis. Let's break this down step by step.

Understanding the Electrolysis Process

In electrolysis, ions in a solution are reduced or oxidized at the electrodes when an electric current passes through. In this case, we are focusing on the reduction of Fe³⁺ ions to solid iron (Fe) at the cathode.

Key Concepts

• Faraday's Law of Electrolysis: The amount of substance deposited or liberated at an electrode during electrolysis is directly proportional to the quantity of electricity passed through the solution.
• Faraday's Constant: This constant (approximately 96485 C/mol) represents the charge required to deposit one mole of a substance. For iron, the reduction reaction is:

Fe³⁺ + 3e^- → Fe

Calculating Moles of Iron Deposited

From the reduction reaction, we see that it takes 3 moles of electrons (3e^-) to reduce 1 mole of Fe³⁺ to solid iron. Now, let's calculate how many moles of electrons are provided by 0.2 Faraday of charge.

Step-by-Step Calculation

1. **Convert Faraday to Moles of Electrons:**

Since 1 Faraday corresponds to 1 mole of electrons, 0.2 Faraday corresponds to:

0.2 moles of electrons.

2. **Determine Moles of Iron Deposited:**

Using the stoichiometry from the reduction reaction, we know that:

1 mole of Fe requires 3 moles of electrons.

Thus, the moles of iron deposited can be calculated as follows:

Let x be the moles of iron deposited:

3x = 0.2 moles of electrons

Solving for x gives:

x = 0.2 / 3 = 0.0667 moles of iron.

Final Result

Therefore, when 0.2 Faraday of charge is passed through the solution, approximately 0.0667 moles of iron will be deposited at the cathode. This calculation illustrates the relationship between charge, moles of electrons, and the amount of substance deposited during electrolysis, which is fundamental in electrochemistry.