(a) Molten NaF is subjected to electrolysis. One of the half-reactions is 2 F- → 2 e- + F2 (g) How many faradays of electricity are required to produce 4.26 L of F2 at 742 torr and 20 °C? (b) If a current of 2.25 A is used, how many hours will it take to carry out the electrolysis in part (a)?
temperature = 20 + 273 = 293 K
pressure = 742 torr = .9763 atm
volume = V = 4.26 L
P V = n R T
.9763 x 4.26 = n x 0.0821 x 293
n = 0.173
2F- ---------------------> F2 + 2e-
1 mole F2 ---------------> 2 F electricity
0.173 mole F2 -------------> 2 x 0.173 = 0.3458 F
number of faradays = 0.3458 F
b)
q = 0.3458 F = 0.3458 x 96500 C = 33368.71 C
i = 2.25 A
i = q / t
2.25 = 33368.71 / t
t = 14830.54 sec
t = 8363 / 3600
t = 2.32 hours
(a) Molten NaF is subjected to electrolysis. One of the half-reactions is 2 F- → 2...
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