The number of moles of potassium iodide required to produce two moles of P is ____.
Correct Answer: 2
Approach Solution - 1
Reaction and Mole Calculation
Step 1: Reaction Equation
The balanced chemical reaction is:
\[ 2 \text{KI} + 2 \text{K}_3[\text{Fe(CN)}_6] \xrightarrow{\text{H}^+} \text{I}_2 + 2 \text{K}_4[\text{Fe(CN)}_6] \]
Step 2: Mole Calculation
From the reaction, 2 moles of KI react with 2 moles of \( \text{K}_3[\text{Fe(CN)}_6] \) to produce 1 mole of \( \text{I}_2 \) and 2 moles of \( \text{K}_4[\text{Fe(CN)}_6] \).
The stoichiometric ratio between KI and \( \text{K}_3[\text{Fe(CN)}_6] \) is 1:1.
If 2 moles of \( \text{K}_3[\text{Fe(CN)}_6] \) are used, 2 moles of KI are required.
Approach Solution -2
To solve the problem, we need to determine the number of moles of potassium iodide required to produce 2 moles of complex \( P \) when potassium iodide reacts with potassium ferricyanide.
1. Reaction and complex formation:
- Potassium ferricyanide: \( \mathrm{K_3[Fe(CN)_6]} \)
- Potassium iodide: \( \mathrm{KI} \)
- Reaction forms complex \( P \) reversibly.
- In strong acidic medium, equilibrium shifts completely towards \( P \).
2. Stoichiometry:
- The complex \( P \) is formed by the reaction of potassium ferricyanide with potassium iodide.
- Each mole of potassium ferricyanide requires 1 mole of potassium iodide to form 1 mole of complex \( P \) (typical for such redox/complex formation reactions).
- To form 2 moles of \( P \), 2 moles of potassium iodide are required.
Final Answer:
The number of moles of potassium iodide required to produce 2 moles of \( P \) is \(\boxed{2}\).
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