PART B QN 1 PLS SOLVE .

Oxidation of K [Fe(CN),] by an oxidising agent is taking place to yield Fe**, CO₂ and NO. If the oxidising agent is K₂Cr₂O, then how many moles of K₂Cr₂O, reacts with

0.6 mole of K [Fe(CN),] ?

To solve the problem of how many moles of K₂Cr₂O₇ react with 0.6 moles of K[Fe(CN)₆], we first need to understand the chemical reaction that occurs during the oxidation process. In this case, K[Fe(CN)₆] is oxidized to yield Fe²⁺, CO₂, and NO. The potassium dichromate (K₂Cr₂O₇) acts as the oxidizing agent. Let's break down the reaction step by step.

Understanding the Reaction

The oxidation of K[Fe(CN)₆] involves the transfer of electrons from the iron complex to the dichromate ion. The balanced reaction can be represented as follows:

Oxidation Half-Reaction

The oxidation of K[Fe(CN)₆] can be simplified to:

• K[Fe(CN)₆] → Fe²⁺ + CO₂ + NO + electrons

Reduction Half-Reaction

For the reduction of dichromate, the half-reaction is:

• Cr₂O₇²⁻ + 14H⁺ + 6e⁻ → 2Cr³⁺ + 7H₂O

Balancing the Overall Reaction

To balance the overall reaction, we need to ensure that the number of electrons lost in the oxidation half-reaction equals the number of electrons gained in the reduction half-reaction. For every mole of K[Fe(CN)₆] oxidized, we can assume it loses 6 electrons (as per the stoichiometry of the reaction). Therefore, we can set up the following relationship:

• 1 mole of K[Fe(CN)₆] reacts with 1 mole of K₂Cr₂O₇ (which provides 6 electrons).

Calculating Moles of K₂Cr₂O₇

Given that we have 0.6 moles of K[Fe(CN)₆], we can determine the moles of K₂Cr₂O₇ required:

• 0.6 moles of K[Fe(CN)₆] will require 0.6 moles of K₂Cr₂O₇.

Final Answer

Thus, the amount of K₂Cr₂O₇ that reacts with 0.6 moles of K[Fe(CN)₆] is 0.6 moles.

This stoichiometric relationship is crucial in understanding how reactants interact in a chemical reaction, especially when dealing with redox reactions where electron transfer is involved. If you have any further questions about this topic or related concepts, feel free to ask!