What happens to the potential for a half equation when you increase the surface area of an platinum electrode?

answer:

this redox reaction occurs at a platinized platinum electrode. the electrode is dipped in an acidic solution and pure hydrogen gas is bubbled through it. the concentration of both the reduced form and oxidised form is maintained at unity. that implies that the pressure of hydrogen gas is 1 bar (100 kpa) and the activity coefficient of hydrogen ions in the solution is unity. the activity of hydrogen ions is their effective concentration, which is equal to the formal concentration times the activity coefficient. these unit-less activity coefficients are close to 1.00 for very dilute water solutions, but usually lower for more concentrated solutions. the nernst equation should be written as:

explanation:

this redox reaction occurs at a platinized platinum electrode. the electrode is dipped in an acidic solution and pure hydrogen gas is bubbled through it. the concentration of both the reduced form and oxidised form is maintained at unity. that implies that the pressure of hydrogen gas is 1 bar (100 kpa) and the activity coefficient of hydrogen ions in the solution is unity. the activity of hydrogen ions is their effective concentration, which is equal to the formal concentration times the activity coefficient. these unit-less activity coefficients are close to 1.00 for very dilute water solutions, but usually lower for more concentrated solutions. the nernst equation should be written as:

answer: the potential increases with increase in the area

explanation:

more info ? ? i don't understand what the question is

explanation: