`I^(-)(aq.)+MnO_(4)^(-)(aq.)overset(H^(+))toX+Mn^(2+)(aq.)`
`I^(-)(aq.)+MnO_(4)^(-)(aq.) underset("weakly "OH^(-))overset("Neutral or")to Y+MnO_(2)`
`MnO_(4)^(-)(aq.)+Mn^(2+)(aq.) overset(ZnSO_(4)) to Z+4H^(+)`
Product X, Y and Z are respectively.

Options

A. `I_(2),IO_(3)^(-),MnO_(2)`
B. `IO_(3)^(-),I_(2),MnO_(2)`
C. `I_(2),IO_(3)^(-),MnO_(4)^(2-)`
D. `IO_(3)^(-),I_(2),MnO_(4)^(2-)`

Explanation

To solve the given question, we need to analyze the reactions step by step and identify the products X, Y, and Z based on the provided information.

### Step 1: Analyzing the first reaction
The first reaction is:
\[ I^{-} (aq) + MnO_{4}^{-} (aq) \overset{H^{+}}{\rightarrow} X + Mn^{2+} (aq) \]

- In acidic medium, the permanganate ion (\(MnO_{4}^{-}\)) acts as a strong oxidizing agent.
- The iodide ion (\(I^{-}\)) will be oxidized to iodine (\(I_{2}\)).
- The \(MnO_{4}^{-}\) will be reduced to \(Mn^{2+}\).

Thus, the product \(X\) is:
\[ X = I_{2} \]

### Step 2: Analyzing the second reaction
The second reaction is:
\[ I^{-} (aq) + MnO_{4}^{-} (aq) \underset{\text{weakly } OH^{-}}{\rightarrow} Y + MnO_{2} \]

- In a neutral or weakly basic medium, \(MnO_{4}^{-}\) is still an oxidizing agent, but it oxidizes iodide (\(I^{-}\)) to iodate (\(IO_{3}^{-}\)).
- The \(MnO_{4}^{-}\) is reduced to manganese dioxide (\(MnO_{2}\)).

Thus, the product \(Y\) is:
\[ Y = IO_{3}^{-} \]

### Step 3: Analyzing the third reaction
The third reaction is:
\[ MnO_{4}^{-} (aq) + Mn^{2+} (aq) \overset{ZnSO_{4}}{\rightarrow} Z + 4H^{+} \]

- This reaction involves the permanganate ion reacting with manganese in the +2 oxidation state.
- This is a disproportionation reaction where \(MnO_{4}^{-}\) (Mn in +7 oxidation state) and \(Mn^{2+}\) (Mn in +2 oxidation state) yield manganese in the +4 oxidation state, which is \(MnO_{2}\).

Thus, the product \(Z\) is:
\[ Z = MnO_{2} \]

### Summary of Products
- \(X = I_{2}\)
- \(Y = IO_{3}^{-}\)
- \(Z = MnO_{2}\)

### Final Answer
The products \(X\), \(Y\), and \(Z\) are:
- \(X = I_{2}\)
- \(Y = IO_{3}^{-}\)
- \(Z = MnO_{2}\)