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Sagot :
In the electrolysis of water, will it take to produce 235.0 l of H₂ at 1.0 atm and 273 k using an electrolytic cell through which the current is 221.0 mA is 25448 hour.
The ideal gas equation is given as :
P V = n RT
pressure , P = 1 atm
volume , V = 235.0 L
temperature , T = 273 K
gas constant, R = 0.082 atm L /mol K
n = P V / R T
n = (1 × 235 ) / ( 273 × 0.082)
n = 10.49 mol
the reaction is given as :
2H⁺ + 2e⁻ ----> H₂
number of electrons = 2
1 mole of electron = 96500 C
10.49 of electron = 10.49 × 2 × 96500
= 2024570 C
I = 221 mA = 0.221 C/s
q = It
t = q / I
t = 2024570 / 0.221
t = 9160950 s
t = 25448 hour
Thus, in the electrolysis of water, the tike taken is 25448 hour.
To learn more about electrolysis here
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