A current of 7.49×104
A is passed through an electrolysis cell
containing molten NaCl for 9.40
days.
(a) How many grams of sodium are
produced?
g
(b) How many liters of chlorine
are collected, if the gas is at a temperature of
273 K and a pressure of 1.00
atm?
L
a.
Na^+ (aq) + e^- ------------> Na(s)
Z = 1
M = 23g/mole
C = 7.49×104 A
t = 9.4 days = 9.4*24*60*60 = 812160sec
W = MCt/ZF
W = 23*7.49*10^4 *812160/(1*96500) = 14498529g
b.
2Cl^- (aq) -------------. Cl2(g) + 2e^-
Z = 2
W = MCt/ZF
W/M = Ct/ZF
n = Ct/ZF [ n = W/M]
n = 7.49*10^4 *812160/(2*96500) = 315185moles
1 mole of any at STP condition ( 273K, 1atm) occupied volume is 22.4L
315185 moles of any STP (273K,1atm) occupied volume = 22.4*315185/1 = 7060144L
A current of 7.49×104 A is passed through an electrolysis cell containing molten NaCl for 9.40...
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