Calculate the standard reduction potential of the following half cell
`S^(2-)|CuS|Cu`
Given: `K_(sp)(CuS)=10^(-35)andE_(Cu^(2+)//Cu)^(@)=0.34V`

Explanation

To calculate the standard reduction potential of the half-cell \( S^{2-} | CuS | Cu \), we will follow these steps:

### Step 1: Understand the Components
We have the half-cell reaction involving copper sulfide (CuS) and the copper ion (Cu²⁺). The solubility product constant \( K_{sp} \) for CuS is given as \( 10^{-35} \) and the standard reduction potential for the copper half-cell \( E^{\circ}_{Cu^{2+}/Cu} \) is given as \( 0.34 \, V \).

### Step 2: Write the Dissociation Reaction
The dissociation of copper sulfide can be represented as:
\[
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