Consider these two entries from a fictional table of standard reduction potentials. X3+ + 3 e → X(s) E° = -1.87V Y3+ + 3 e Y(s) E° = -0.26 V What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? V 'cell

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**Title: Understanding Galvanic Cell Potential**

Consider these two entries from a fictional table of standard reduction potentials:

\[ \text{X}^{3+} + 3 \, \text{e}^- \rightarrow \text{X(s)} \quad E^\circ = -1.87 \, \text{V} \]

\[ \text{Y}^{3+} + 3 \, \text{e}^- \rightarrow \text{Y(s)} \quad E^\circ = -0.26 \, \text{V} \]

**Question:**

What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode?

\[ E^\circ_{\text{cell}} = \]

**Instructions:**

To calculate the standard cell potential (\(E^\circ_{\text{cell}}\)), use the following formula:
\[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \]

**Solution:**

1. Identify the cathode and anode reactions:
   - Cathode: \( \text{Y}^{3+} + 3 \, \text{e}^- \rightarrow \text{Y(s)} \) with \( E^\circ = -0.26 \, \text{V} \)
   - Anode: \( \text{X}^{3+} + 3 \, \text{e}^- \rightarrow \text{X(s)} \) with \( E^\circ = -1.87 \, \text{V} \)

2. Apply the formula:
   \[ E^\circ_{\text{cell}} = (-0.26 \, \text{V}) - (-1.87 \, \text{V}) = 1.61 \, \text{V} \]

Therefore, the standard potential of the galvanic cell is 1.61 V.

\[ E^\circ_{\text{cell}} = 1.61 \, \text{V} \]
Transcribed Image Text:**Title: Understanding Galvanic Cell Potential** Consider these two entries from a fictional table of standard reduction potentials: \[ \text{X}^{3+} + 3 \, \text{e}^- \rightarrow \text{X(s)} \quad E^\circ = -1.87 \, \text{V} \] \[ \text{Y}^{3+} + 3 \, \text{e}^- \rightarrow \text{Y(s)} \quad E^\circ = -0.26 \, \text{V} \] **Question:** What is the standard potential of a galvanic (voltaic) cell where X is the anode and Y is the cathode? \[ E^\circ_{\text{cell}} = \] **Instructions:** To calculate the standard cell potential (\(E^\circ_{\text{cell}}\)), use the following formula: \[ E^\circ_{\text{cell}} = E^\circ_{\text{cathode}} - E^\circ_{\text{anode}} \] **Solution:** 1. Identify the cathode and anode reactions: - Cathode: \( \text{Y}^{3+} + 3 \, \text{e}^- \rightarrow \text{Y(s)} \) with \( E^\circ = -0.26 \, \text{V} \) - Anode: \( \text{X}^{3+} + 3 \, \text{e}^- \rightarrow \text{X(s)} \) with \( E^\circ = -1.87 \, \text{V} \) 2. Apply the formula: \[ E^\circ_{\text{cell}} = (-0.26 \, \text{V}) - (-1.87 \, \text{V}) = 1.61 \, \text{V} \] Therefore, the standard potential of the galvanic cell is 1.61 V. \[ E^\circ_{\text{cell}} = 1.61 \, \text{V} \]
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