Two half cell reactions of an electrochemical cell are given below :
`MnO_(4)^(-)(aq)+8H^(+)(aq)+5e^(-),toMn^(2+)(aq)+4H_(2)O(l),E^(@)=+1.51V`
`Sn^(2+)(aq)toSn^(4+)(aq)+2e^(-),E^(@)=+0.51V` 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 solve the problem, we will follow these steps:

### Step 1: Write the two half-reactions
We have the following half-reactions:
1. Reduction half-reaction:
\[ \text{MnO}_4^{-} + 8\text{H}^{+} + 5\text{e}^{-} \rightarrow \text{Mn}^{2+} + 4\text{H}_2\text{O}, \quad E^{\circ} = +1.51 \, \text{V} \]
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