What is the standard cell potential (E°_cell) for the voltaic cell represented by the following cell diagram? Pt | H2(g, 1 atm) | 0.0025 M HCl || H+ (1 M) | H2(g, 1 atm) | Pt

• A. 0.50 V
• B. 0.00 V
• C. 0.25 V
• D. 0.12 V

Answer: (B)

Verified step by step guidance

1. Identify the half-reactions involved in the cell. In this case, both half-reactions involve the hydrogen electrode: H2(g) ⇌ 2H+(aq) + 2e−.
2. Determine the standard reduction potential for the hydrogen electrode. The standard hydrogen electrode (SHE) has a potential of 0.00 V.
3. Since both electrodes are hydrogen electrodes, the standard cell potential (E°_cell) is calculated as the difference between the cathode and anode potentials. Here, both are 0.00 V.
4. Calculate the standard cell potential using the formula: E°_cell = E°_cathode - E°_anode. Substitute the values: E°_cell = 0.00 V - 0.00 V.
5. Conclude that the standard cell potential (E°_cell) for this cell is 0.00 V, as both electrodes are identical and have the same potential.