The following reaction`:` occurs in the dry cell, called flash light battery, which is used to power radios, clocks, and flashlights `:`
`2MnO_(2)(s)+8overset(o+)(N)H_(4)+Zn(s) rarr 2Mn^(3+)+8NH_(3)+Zn^(2+)+4H_(2)O`
`a.` Write the anode and cathode reactions.
`b.` Calculate `E^(c-)._(cell)` of the dry cell if the electrode potential of cathode `(E^(c-)._(reduction ))` varies between `0.49V` and `0.74V` and that of anode `E^(c-)._(reduction) ` is `-0.76V`.

Explanation

To solve the given problem, we will break it down into two parts as requested.

### Part a: Write the anode and cathode reactions.

1. **Identify the Anode Reaction:**
- In the dry cell reaction, oxidation occurs at the anode.
- The zinc (Zn) is oxidized to zinc ions (Zn²⁺) by losing electrons.
- The half-reaction at the anode can be written as:
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