This means that two electrons would be transferred in each half reaction for

# This means that two electrons would be transferred in

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of those reactions as well. This means that two electrons would be transferred in each half reaction for one mole of water. The experimental number of electrons transferred is found by multiplying the average current by the time the current ran in seconds, which is equal to the coulombs of charge that passed through the solution. Then you divide this amount by the moles of hydrogen gas (which is equal to the moles of water) multiplied by 96,485. 96,485 is Faraday’s constant, which is equal to the coulombs per mole of an electron. On the bottom of the equation you have units of coulombs/ e - * mol of H 2 O. This is equal to mol of H 2 O * coulombs over e - . When you bring the denominator of the equation to the numerator you get coulombs * e - over mol of H 2 O * coulombs. The coulombs cancel out and you get e - over mol of H 2 O or electrons per mole of water. Reference equation: e ¿ mol H 2 O e ¿ coulombs ¿ ¿ 96,485 ¿ ¿ = Q ( coulombs ) ¿ z ¿
E. Reflection How did the number of electrons transferred during the reaction that you measured compare to that which should have theoretically been transferred? What may account for any differences? The experimentally determined number of electrons transferred during my electrolysis of water reaction was 2.19, while the theoretical value of transferred electrons for this reaction should have been 2. The experimental value that I obtained has a percent error

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