Question

How many faradays of electricity are involved when 5.0 l of o2 at stp is converted to h20 in acid solution?

Answer 1

0.893 Faraday

Step-by-step explanation:

Hello,

In this case, the undergoing chemical reaction is given as follows:

`O_2+4H^+-->2H_2O`

Now, the oxygen's half-reaction turn out into:

`O_2^0-->O^(-2)+4e^-`

Let us identify that four electrons were involved since there are two oxygens that transfer two electrons for a total of four. In such a way, to compute the faradays of electricity, one multiplies the changing moles by the amount of transferred electrons as shown below:

`Electricity=n*e^-=(PV)/(RT)*e^-=(1atm*5.0L)/(0.082 (atm*L)/(mol*K) * 273.15K)*4\\Electricity=0.893Faraday`

Best regards.

Answer 2

2 O₂ + 4 H⁺ → 2 H₂O

So 5 L of O₂ = 5 L / 22.4 L per one mole = 0.22 mol O₂

Since the mole ratio is constant, you don't have to multiply because of that. However, O₂ is reduced to a -2 oxidation number.

So 2 (0.22 mol) = 0.44 mol of electrons = 0.44 Faraday