Answer : The number of faradays of electricity had to pass through the solution will be, 0.596 F
Explanation :
First we have to calculate the moles of oxygen gas.
using ideal gas equation:
[tex]PV=nRT[/tex]
where,
P = pressure of gas = 755 mm Hg = 0.99 atm
conversion used : (1 atm = 760 mmHg)
V = volume of gas = 3.696 L
T = temperature of gas = [tex]25^oC=273+25=298K[/tex]
n = number of moles of gas = ?
R = gas constant = 0.0821 L.atm/mole.K
Now put all the given values in the ideal gas equation, we get the number of moles of oxygen gas.
[tex](0.99atm)\times (3.696L)=n\times (0.0821L.atm/mole.K)\times (298K)[/tex]
[tex]n=0.149mole[/tex]
Now we have to calculate the number of faradays of electricity had to pass through the solution.
The balanced half-reactions for the electrolysis of water is,
[tex]2H_2O(l)\rightarrow O_2(g)+4H^+(aq)+4e^-[/tex]
From this we conclude that,
As, 1 mole of oxygen gas require 4 mole of electrons that means 4 F (faraday) of electricity.
So, 0.149 mole of oxygen gas require [tex]0.149\times 4=0.596F[/tex] of electricity.
Therefore, the number of faradays of electricity had to pass through the solution will be, 0.596 F
