1384/63.5 moles = 0.00218 molesThe ratio of moles of Cu dissolved to the moles of H2 produced is ~ 1:1 as we would expect from the equation.# of Coulombs = current x time = 0.73 x 603 = 440.19 CThis is the amount of electricity which dissolved 0.......
substituting the values of p, V and T in (1) we get # moles H2 = 0.00221 moles
moles of Cu dissolved = 23.0425 - 22.9041 = 0.1384 g = 0.1384/63.5 moles = 0.00218 moles
The ratio of moles of Cu dissolved to the moles of H2 produced is ~ 1:1 as we would expect from the equation.
# of Coulombs = current x time = 0.73 x 603 = 440.19 C
This is the amount of electricity which dissolved 0.00218 moles of Cu and hence Charge /mole of e
= 440.19/ (2 x 0.00218) = 100982 Coulombs where we divide by 2 because oxidation of Cu involves loss of 2 electrons. Accepted value = 96500 C; error ~ 4.64%
Exptal Avogadro # = 100982/(1.602 x 10^-19) = 6.303 x 10^23
You have to have the formula once you have them you can attempt it on your own.
Q = IT , F=LE and Q=nF. Q is the energy required I is current in ampere F is faraday which can be found in the data booklet and usually if its unknown we take it that its 965000. t is the time L is avogadro constant and e is charge of electron which can also be found in the data booklet. this is actually quite simple once u have the formula.
