Enter your answer in the provided box. one of the half-reactions for the electrolysis of water is 2h2o(l) → o2(g) + 4h+(aq) + 4e− if 3.696 l of o2 is collected at 25°c and 755 mmhg, how many faradays of electricity had to pass through the solution?

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:

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 =

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.

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,

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 of electricity.

Therefore, the number of faradays of electricity had to pass through the solution will be, 0.596 F

h let me think

2h2o2--> 2h2o + o2

this reaction is of the spontaneous decomposition of hydrogen peroxide down into water and oxygen.

add 2 molecules of hydrogen peroxide and 2 molecules of water. since oxygen is naturally diatomic, the total number of atoms of each element is now the same on both sides of the equation so it is balanced.

this may not be entirely correct but let me know.