Two half-reactions of an electrochemical cell are given below :
`MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-) toMn^(2+)(aq)+4H_(2)O(l), E^(@)=+1.51" V"`
`Sn^(2+)(aq) to Sn^(4+)(aq)+2e^(-),E^(@)=-0.15" V"`
Construct the redox equation from the two half cell reactions and predict if the reaction favours formation of reactant or product shown in the equation.

Explanation

To construct the redox equation from the two half-cell reactions and predict whether the reaction favors the formation of reactants or products, we can follow these steps:

### Step 1: Identify the half-reactions
We have two half-reactions:
1. \( \text{MnO}_4^{-} + 8\text{H}^{+} + 5\text{e}^{-} \rightarrow \text{Mn}^{2+} + 4\text{H}_2\text{O} \) with \( E^{\circ} = +1.51 \, \text{V} \)
2. \( \text{Sn}^{2+} \rightarrow \text{Sn}^{4+} + 2\text{e}^{-} \) with \( E^{\circ} = -0.15 \, \text{V} \)

### Step 2: Balance the electron transfer
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