Two galvanic cells were constructed under standard conditions in an experiment to determine the relative positions in the electrochemical series of the standard electrode potential, $E^\circ$, for the following reactions. Both cells generate a potential difference. 1. $\text{Ag(NH}_3)_2^+(aq) + e^- \rightleftharpoons \text{Ag}(s) + 2\text{NH}_3(aq) \quad E_1$ 2. $\text{Ag}^+(aq) + e^- \rightleftharpoons \text{Ag}(s) \quad E_2$ 3. $\text{Ag(CN)}_2^-(aq) + e^- \rightleftharpoons \text{Ag}(s) + 2\text{CN}^-(aq) \quad E_3$ The values of the electrode potentials in order from highest to lowest would be: A. $E_1, E_2, E_3$ B. $E_2, E_1, E_3$ C. $E_3, E_2, E_1$ D. $E_1, E_3, E_2$

SSCE VCE Chemistry Primary Galvanic Cells and Fuel Cells as Sources of Energy: Two galvanic cells were construc

Two galvanic cells were constructed under standard conditions in an experiment to determine the relative positions in the electrochemical series of the standard electrode potential, $E^\circ$, for the following reactions - VCE - SSCE Chemistry - Question 10 - 2011 - Paper 1

Question 10

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Two galvanic cells were constructed under standard conditions in an experiment to determine the relative positions in the electrochemical series of the standard elec... show full transcript

Worked Solution & Example Answer:Two galvanic cells were constructed under standard conditions in an experiment to determine the relative positions in the electrochemical series of the standard electrode potential, $E^\circ$, for the following reactions - VCE - SSCE Chemistry - Question 10 - 2011 - Paper 1

Step 1

Determine the Electrode Reactions

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Answer

The first step is to analyze the three given electrode reactions thoroughly. From the chemical equations, identify the associated standard electrode potentials $E^\circ$ for each reaction:

$E_1$ : Reduction of $\text{Ag(NH}_3)_2^+$ to solid Ag.
$E_2$ : Reduction of $\text{Ag}^+$ to solid Ag.
$E_3$ : Reduction of $\text{Ag(CN)}_2^-$ to solid Ag.

Understanding these reactions helps us to predict their potentials.

Step 2

Analyze the Stability based on Complexing Agents

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In the series, complex formation generally increases the stability of the metal ion. Given that the silver ion is more stabilized when complexed with cyanide compared to ammonia, we can infer:

$\text{Ag(CN)}_2^-$ is likely to have the lowest potential ( $E_3$ ).
$\text{Ag(NH}_3)_2^+$ provides more potential than cyanide but less than the free ion since ammonia is a weaker ligand than cyanide, thus $E_1 < E_2$ .

Step 3

Rank the Electrode Potentials

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Using the information gathered, we rank the potentials in descending order:

Free $\text{Ag}^+ \quad (E_2)$
$\text{Ag(NH}_3)_2^+ \quad (E_1)$
$\text{Ag(CN)}_2^- \quad (E_3)$

Thus, the correct order from highest to lowest is $E_2 > E_1 > E_3$ .

Step 4

Final Answer Selection

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From the ranks, the correct choice from the options provided is:

C. $E_3, E_2, E_1$

Two galvanic cells were constructed under standard conditions in an experiment to determine the relative positions in the electrochemical series of the standard electrode potential, $E^\circ$, for the following reactions - VCE - SSCE Chemistry - Question 10 - 2011 - Paper 1

Determine the Electrode Reactions

Analyze the Stability based on Complexing Agents

Rank the Electrode Potentials

Final Answer Selection

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