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The cell, Zn | Zn^(2+) (1M) || (1M) | Cu...

The cell, `Zn | Zn^(2+) (1M) || (1M) | Cu (E_(cell)^(@) = 1.10V)`, was was allowed to be completely discharged at 298 K. The concentration of `Zn^(2+)` `rightarrow CU^(2+)([([Zn^(2+)]/([Cu^(2+)])])` is :

A

antilog(24.08)

B

37.3

C

`10^(37.3)`

D

`9.65xx10^(4)`

Text Solution

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To solve the problem, we will use the Nernst equation, which relates the cell potential to the concentrations of the reactants and products in an electrochemical cell. ### Step-by-Step Solution: 1. **Identify the Components of the Cell**: The given cell is represented as `Zn | Zn^(2+) (1M) || (1M) | Cu`. This indicates that zinc is being oxidized to zinc ions (Zn → Zn²⁺) and copper ions (Cu²⁺) are being reduced to copper (Cu). 2. **Write the Half-Reactions**: ...
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