The standard electrode potentials \( E^\circ (V) \) for \( Li^+/Li \), \( Na^+/Na \) respectively are:
(1) −3.04, −2.714
(2) −2.714, −3.04
(3) −3.04, −3.04
(4) −2.714, −2.714
The standard electrode potentials \( E^\circ (V) \) for \( Li^+/Li \), \( Na^+/Na \) respectively are:
(1) −3.04, −2.714
(2) −2.714, −3.04
(3) −3.04, −3.04
(4) −2.714, −2.714
Show Hint
- \( -3.04, -2.714 \)
- \( -2.714, -3.04 \)
- \( -3.04, -3.04 \)
\( -2.714, -2.714 \)
The Correct Option is A
Solution and Explanation
Step 1: Understanding Standard Electrode Potential
The standard electrode potential (\( E^\circ \)) of an element is a measure of the tendency of the element to gain or lose electrons in an electrochemical reaction. It is given in volts (\( V \)) and is measured under standard conditions.
Step 2: Standard Electrode Potentials for Lithium and Sodium
- For lithium, the standard reduction potential is: \[ Li^+ + e^- \rightarrow Li, \quad E^\circ = -3.04V \] - For sodium, the standard reduction potential is: \[ Na^+ + e^- \rightarrow Na, \quad E^\circ = -2.714V \]
Step 3: Evaluating the Given Options
- Option (1): \( -3.04, -2.714 \) Correct as per standard data.
- Option (2): \( -2.714, -3.04 \) Incorrect as the values are reversed.
- Option (3): \( -3.04, -3.04 \) Incorrect as the value for sodium is wrong.
- Option (4): \( -2.714, -2.714 \) Incorrect as the value for lithium is wrong.
Thus, the correct answer is
Option (1).
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