1 mole of `H_(3) PO_(2)` reacts completely to two moles of `I_(2)`. `I_(2)` converts to `I^(-)` , what will be the oxidation state of P in the product?

Answer

To determine the oxidation state of phosphorus (P) in the product formed from the reaction of 1 mole of H₃PO₂ with 2 moles of I₂, we will follow these steps:

### Step 1: Identify the reactants and products
The reactants are:
- H₃PO₂ (phosphorous acid)
- I₂ (iodine)

The product formed from this reaction is H₃PO₄ (phosphoric acid) and I⁻ (iodide ion).

### Step 2: Write the balanced reaction
The balanced chemical reaction can be written as:
\[ \text{H}_3\text{PO}_2 + 2 \text{I}_2 \rightarrow \text{H}_3\text{PO}_4 + 2 \text{I}^- \]

### Step 3: Determine the oxidation state of phosphorus in H₃PO₄
To find the oxidation state of phosphorus in H₃PO₄, we can use the following formula based on the known oxidation states of hydrogen and oxygen:

Let the oxidation state of phosphorus be \( x \).
- The oxidation state of hydrogen (H) is +1.
- The oxidation state of oxygen (O) is -2.

The formula for the compound H₃PO₄ can be set up as follows:
\[ 3(+1) + x + 4(-2) = 0 \]

### Step 4: Solve for x
Now, substituting the values:
\[ 3(1) + x + 4(-2) = 0 \]
\[ 3 + x - 8 = 0 \]
\[ x - 5 = 0 \]
\[ x = +5 \]

### Conclusion
Thus, the oxidation state of phosphorus (P) in the product H₃PO₄ is +5.