What is the reduction potential of a hydrogen electrode that is still at standard pressure, but has ph = 5.65 , relative to the she?

Explanation:

We must use the Nernst equation

1. Write the equation for the cell reaction

If you want the reduction potential, the pH 5.65 solution is the cathode, and the cell reaction is

                                                                      E°/V

  Anode: H₂(1 bar) ⇌ 2H⁺(1 mol·L⁻¹) + 2e⁻;     0

Cathode: 2H⁺(pH 5.65) + 2e⁻ ⇌ H₂(1 bar);     0

 Overall: 2H⁺ (pH 5.65) ⇌ 2H⁺(1 mol·L⁻¹);      0

Step 2. Calculate E°

(a) Data

   E° = 0

   R = 8.314 J·K⁻¹mol⁻¹

   T = 25 °C

   n = 2

   F = 96 485 C/mol

pH = 5.65

Calculations:  

T = 25 + 273.15 = 298.15 K

the old alchemists made significant contributions to science even though there starting premises were off a bit. their conclusions after failure would steer them into better directions for investigation. science is no more than close observation and the initial mistakes result in rethinking and retrying experiments.

the correct answer is option d

explanation:

i was wrong its d because they dont use cm when calculating square roots