Two half-reactions of an electrochemical cell are given below:
`MnO_(4)^(-)(aq) +8H^(+) (aq) +5e^(-) to Mn^(2+)(aq) +4H_(2)O(l), E^(Theta)= +1.51V`
`Sn^(2+)(aq) to Sn^(4+)(aq)+2e^(-), E^(Theta)=0.15V`
Construct the redox reaction equation from the two half reactions and calculate the cell potential from the standard potentials and predict if the reaction is reactant or product favoured.

Explanation

To solve the problem, we will follow these steps:

### Step 1: Write the Half-Reactions
We are given two half-reactions:
1. Reduction half-reaction:
\[ \text{MnO}_4^{-} (aq) + 8H^{+} (aq) + 5e^{-} \rightarrow \text{Mn}^{2+} (aq) + 4H_2O (l), \quad E^{\Theta} = +1.51 \, V \]
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