A hydrogen gas electrode is made by dipping platinum wire in a solution of HCl of pH=10 and by passing hydrogen gas around the platinum wire at 1 atm pressure. The oxidation potential of electrode would be

To determine the oxidation potential of the hydrogen gas electrode, we need to follow these steps:

Step 1: Understand the setup

• The hydrogen gas electrode is made by dipping a platinum wire in a solution of HCl with a pH of 10.
• Hydrogen gas is passed around the platinum wire at a pressure of 1 atm.

Step 2: Identify the half-reaction

• In this case, the half-reaction is the oxidation of hydrogen gas (H2) to form hydrogen ions (H+).
• The balanced half-reaction is: H2(g) -> 2H+(aq) + 2e-

Step 3: Determine the standard reduction potential

• The standard reduction potential for the half-reaction can be found in a standard reduction potential table.
• The standard reduction potential for the reduction of H+ to H2 is 0.00 V.

Step 4: Apply the Nernst equation

• The Nernst equation allows us to calculate the oxidation potential of the electrode under non-standard conditions.
• The Nernst equation is: E = E° - (0.0592/n) * log(Q)
  • E is the oxidation potential
  • E° is the standard reduction potential
  • n is the number of electrons transferred in the half-reaction
  • Q is the reaction quotient, which is the ratio of the concentrations of the products to the concentrations of the reactants

Step 5: Calculate the reaction quotient

• In this case, the reaction quotient (Q) is equal to the concentration of H+ ions raised to the power of 2 (since the balanced half-reaction involves the formation of 2H+ ions) divided by the concentration of H2 gas.
• Since the HCl solution has a pH of 10, the concentration of H+ ions can be calculated using the equation: [H+] = 10^(-pH)
• The concentration of H2 gas is 1 atm.

Step 6: Plug values into the Nernst equation and calculate

• Using the values obtained in the previous steps, we can now calculate the oxidation potential of the hydrogen gas electrode.

Please note that the specific numerical value of the oxidation potential cannot be determined without knowing the exact concentrations of H+ ions and H2 gas.