Question

Calculate the maximum standard voltage possible for a voltaic cell based on the following half reactions: E°/V 2H+(aq)+2e-→H₂(g)0.00 F₂(g)+2e-→2F-(aq)2.87

A. +2.87 V
B. +0.00 V
C. -2.87 V
D. +5.74 V

Answer 1

The maximum standard voltage of the voltaic cell using the given half-reactions is +2.87 V, calculated by subtracting the anode potential (0.00 V) from the cathode potential (2.87 V).

Step-by-step explanation:

The question asks us to calculate the maximum standard voltage of a voltaic cell using given half-reactions. The half-reactions provided are:

• 2H+(aq) + 2e- → H₂(g) with E° = 0.00 V
• F₂(g) + 2e- → 2F-(aq) with E° = 2.87 V

To calculate the standard cell potential (E°cell), we use the formula:

E°cell = E°cathode - E°anode

First, identify the reduction and oxidation reactions. The fluoride ion is reduced as it gains electrons and has a higher reduction potential, so it serves as the cathode. Hydrogen is oxidized at the anode. Using the provided standard reduction potentials:

E°cell = 2.87 V (cathode) - 0.00 V (anode) = +2.87 V

This is the maximum standard voltage possible under standard conditions (1 M concentrations for aqueous species, 1 atm for gases, and a temperature of 25°C).