The coefficient of $I^{-}$, $MnO_{4}^{-}$ and $H_{2}O$ in the redox reaction
$I^{-}(aq)+MnO_{4}^{-}(aq)+H_{2}O(l)\rightarrow I_{2}(s) +MnO_{2}(s)+OH^{-}(aq)$
in the balance form respectively are:

Question

The coefficient of $I^{-}$, $MnO_{4}^{-}$ and $H_{2}O$ in the redox reaction 
$I^{-}(aq)+MnO_{4}^{-}(aq)+H_{2}O(l)\rightarrow I_{2}(s) +MnO_{2}(s)+OH^{-}(aq)$ 
in the balance form respectively are:

Accepted Answer

To determine the correct coefficients for the redox reaction $I^{-}(aq) + MnO_{4}^{-}(aq) + H_{2}O(l) \rightarrow I_{2}(s) + MnO_{2}(s) + OH^{-}(aq)$, we need to balance the reaction by ensuring that both mass and charge are conserved.

### Explanation for Option 3 (Correct Answer: 6, 2, 4)

1. **Balancing the Iodine Atoms:**
   - On the left side, we have iodide ions $I^{-}$.
   - On the right side, iodine is present as $I_{2}$.
   - To balance the iodine atoms, we need 6 iodide ions to form 3 molecules of $I_{2}$: 
     $$
     6I^{-} \rightarrow 3I_{2}
     $$

2. **Balancing the Manganese Atoms:**
   - On the left side, manganese is present as $MnO_{4}^{-}$.
   - On the right side, manganese is present as $MnO_{2}$.
   - To balance the manganese atoms, we need 2 permanganate ions to form 2 molecules of $MnO_{2}$:
     $$
     2MnO_{4}^{-} \rightarrow 2MnO_{2}
     $$

3. **Balancing the Oxygen Atoms:**
   - On the left side, we have 8 oxygen atoms from 2 $MnO_{4}^{-}$ and additional oxygen from water.
   - On the right side, we have 4 oxygen atoms in $MnO_{2}$ and additional oxygen in $OH^{-}$.
   - To balance the oxygen atoms, we need 4 water molecules on the left side to provide the necessary oxygen atoms:
     $$
     4H_{2}O \rightarrow 4OH^{-}
     $$

4. **Balancing the Charge:**
   - On the left side, the total charge is $6 \times (-1) + 2 \times (-1) = -8$.
   - On the right side, the total charge is $4 \times (-1) = -4$.
   - The charges are balanced by ensuring that the number of electrons lost and gained in the redox process is equal.

Thus, the balanced equation is:
$$
6I^{-} + 2MnO_{4}^{-} + 4H_{2}O \rightarrow 3I_{2} + 2MnO_{2} + 4OH^{-}
$$

### Explanation for Why Other Options are Incorrect:

- **Option 1 (3, 5, 4):** 
  - This option suggests using 3 iodide ions and 5 permanganate ions, which does not balance the iodine and manganese atoms correctly. Additionally, the oxygen and charge balance would not be satisfied.

- **Option 2 (Sat Jun 01 2002 12:30:00 GMT+0530 (GMT+05:30)):**
  - This is not a valid set of coefficients; it appears to be a date and time, which is irrelevant to balancing a chemical equation.

- **Option 4 (Sat Apr 03 2004 13:30:00 GMT+0530 (GMT+05:30)):**
  - Similar to Option 2, this is a date and time, not a set of coefficients for balancing the equation.

In conclusion, Option 3 (6, 2, 4) is the correct set of coefficients that balances the redox reaction in terms of both mass and charge.