For the cell: `Zn(s)|ZnSO_(4)(aq)||CuSO_(4)(aq)Cu(s)`, calculate standard cell potential if standard state reduction electrode potentials for `Cu^(2+)//Cu and Zn^(2+)//Zn` are +0.34V and -0.76V respectively.

Answer

To calculate the standard cell potential for the given electrochemical cell \( \text{Zn(s)} | \text{ZnSO}_4(aq) || \text{CuSO}_4(aq) | \text{Cu(s)} \), we will follow these steps:

### Step 1: Identify the half-reactions
In this electrochemical cell:
- The oxidation half-reaction occurs at the anode (zinc side):
\[ \text{Zn} \rightarrow \text{Zn}^{2+} + 2e^- \]
- The reduction half-reaction occurs at the cathode (copper side):
\[ \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \]

### Step 2: Write the standard reduction potentials
From the problem, we have the standard reduction potentials:
- For copper:
\[ E^\circ_{\text{Cu}^{2+}/\text{Cu}} = +0.34 \, \text{V} \]
- For zinc:
\[ E^\circ_{\text{Zn}^{2+}/\text{Zn}} = -0.76 \, \text{V} \]

### Step 3: Determine the standard cell potential
The standard cell potential \( E^\circ_{\text{cell}} \) can be calculated using the formula:
\[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \]
Here, the cathode is where reduction occurs (copper), and the anode is where oxidation occurs (zinc).

Substituting the values:
\[ E^\circ_{\text{cell}} = E^\circ_{\text{Cu}^{2+}/\text{Cu}} - E^\circ_{\text{Zn}^{2+}/\text{Zn}} \]
\[ E^\circ_{\text{cell}} = 0.34 \, \text{V} - (-0.76 \, \text{V}) \]
\[ E^\circ_{\text{cell}} = 0.34 \, \text{V} + 0.76 \, \text{V} \]
\[ E^\circ_{\text{cell}} = 1.10 \, \text{V} \]

### Conclusion
The standard cell potential for the given electrochemical cell is:
\[ E^\circ_{\text{cell}} = 1.10 \, \text{V} \]