Calculate Standard Cell Potential for Zn and Sn Reaction

Math Problem Statement

The standard cell potential for the galvanic cell based on the reaction below is V.

Zn(s) + Sn4+(aq) → Sn2+(aq) + Zn2+(aq)

Half-reaction

E° / V

Sn4+(aq) + 2e- → Sn2+(aq)

0.15

Zn2+(aq) + 2e- → Zn(s)

-0.76

-0.91 0.91 1.45 0.61 -0.61

To calculate the standard cell potential $E^\circ_{\text{cell}}$ for a galvanic cell, we use the formula:

$E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}}$

Given the overall cell reaction:

$\text{Zn(s)} + \text{Sn}^{4+}(aq) \rightarrow \text{Sn}^{2+}(aq) + \text{Zn}^{2+}(aq)$

The oxidation half-reaction (anode):
$\text{Zn(s)} \rightarrow \text{Zn}^{2+}(aq) + 2e^-$
$E^\circ_{\text{anode}} = -0.76 \, V$
The reduction half-reaction (cathode):
$\text{Sn}^{4+}(aq) + 2e^- \rightarrow \text{Sn}^{2+}(aq)$
$E^\circ_{\text{cathode}} = 0.15 \, V$

= 0.15 - (-0.76)$$ $$E^\circ_{\text{cell}} = 0.15 + 0.76 = 0.91 \, V$$ ### Final Answer: The standard cell potential for the galvanic cell is **0.91 V**. Would you like more details or have any questions? ### 5 Related Questions: 1. How does the sign of cell potential relate to the spontaneity of the reaction? 2. What is the significance of standard reduction potentials in a galvanic cell? 3. How can the Nernst equation modify cell potential for non-standard conditions? 4. What role do electrons play in oxidation and reduction half-reactions? 5. How do we determine which electrode acts as the anode or cathode? ### Tip: In a galvanic cell, the electrode where reduction occurs is always the cathode, and the electrode where oxidation occurs is the anode.

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Electrochemistry
Standard Cell Potential
Redox Reactions

E°cell = E°cathode - E°anode

Nernst Equation (for non-standard conditions)

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