Answer:
55.7 hrs
Step-by-step explanation:
We'll begin by calculating the number of mole of O2 produced during the process. This can be obtained as follow:
Volume (V) = 15L
Pressure (P) = 750torr = 750/760 = 0.99atm
Temperature (T) = 30°C = 30°C + 273 = 303K
Gas constant (R) = 0.0821 atm.L/Kmol
Number of mole (n) =?
PV = nRT
0.99 x 15 = n x 0.0821 x 303
Divide both side by 0.0821 x 303
n = (0.99 x 15 ) /(0.0821 x 303)
n = 0.597 mole
Next, we shall determine the quantity of electricity required to liberate 1 mole of O2. This is illustrated below:
2O^2- + 4e —> O2
Thus, 4 moles of electron (e) is needed to produce 1 mole of O2.
Recall:
1 electron (e) = 1 Faraday = 96500C
1e = 96500C
Therefore, 4e = 4 x 96500C = 386000C.
Therefore, 386000C of electricity is required to liberate 1 mole of O2.
Next, we shall determine the quantity of electricity required to liberate 0.597 mole of O2.
This is illustrated below:
From the balanced equation above,
386000C of electricity is required to liberate 1 mole of O2.
Therefore, XC of electricity will be required to liberate 0.597 mole of O2 i.e
XC of electricity = 386000 x 0.597
XC of electricity = 230442C
Therefore, 230442C of electricity is needed to liberate 0.597 mole of O2.
Now, we can obtain the time taken to produce 0.597 mole of O2 as follow:
Current (I) = 1.15A
Quantity of electricity (Q) = 230442C
Time (t) =.?
Q = It
230442 = 1.15 x t
Divide both side by 1.15
t = 230442/1.15
t = 200384.35 secs
Finally, we shall convert 200384.35 secs to hours. This is illustrated below:
3600 secs = 1 hr
Therefore, 200384.35 secs = 200384.35/3600 = 55.7 hrs
Therefore, it will take 55.7 hrs to produce 15L of O2.