Calculate the values of E standard, Delta G standard (in kJ), and K at 25 degree

Question

Calculate the values of E standard, Delta G standard (in kJ), and K at 25 degrees Celcius for the cell reaction in a hydrogen-oxygen fuel cell: 2H2(g) + O2(g) -----> 2H2O (l) Part A asked for E standard, which I found to be 1.23V. Part B asked for Delta G standard, which I found to be -475kJ. Part C asked for the equilbirum constant, which I found to be 1x10^83. Part D is what I can't figure out, maybe it's because I'm tired... who knows. It asks: "What is the cell voltage at 25 degrees Celcius if the partial pressure of each gas is 17atm?" Part D is the only part I need an answer to, obviously ;) Calculate the values of E standard, Delta G standard (in kJ), and K at 25 degrees Celcius for the cell reaction in a hydrogen-oxygen fuel cell: 2H2(g) + O2(g) -----> 2H2O (l) Part A asked for E standard, which I found to be 1.23V. Part B asked for Delta G standard, which I found to be -475kJ. Part C asked for the equilbirum constant, which I found to be 1x10^83. Part D is what I can't figure out, maybe it's because I'm tired... who knows. It asks: "What is the cell voltage at 25 degrees Celcius if the partial pressure of each gas is 17atm?" Part D is the only part I need an answer to, obviously ;)

Explanation / Answer

E cell= E^0 CELL - (0.059/n) log(1/[P H2]^2 * PO2])

E CELL= 1.23-(0.059/4)log1/17^2*17)

ECELL = 1.175 V

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