Given that `E_(Cu^(2+)//Cu)^(0)=0.337` and `E_(Cu^(+)//Cu^(2+))^(0)=-0.153V`. then calculate `E_(Cu^(+)//Cu)^(0)`

Explanation

To calculate \( E^\circ_{Cu^+ // Cu} \) using the given standard electrode potentials \( E^\circ_{Cu^{2+} // Cu} = 0.337 \, V \) and \( E^\circ_{Cu^+ // Cu^{2+}} = -0.153 \, V \), we can follow these steps:

### Step 1: Write the half-reactions
We start with the half-reactions corresponding to the given standard electrode potentials.

1. For \( E^\circ_{Cu^{2+} // Cu} \):
\[
Cu^{2+} + 2e^- \rightarrow Cu \quad (1)
...