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

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

Answer 2

Answer:

0.893 Faraday

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:

$Electricity=n*e^-=\frac{PV}{RT}*e^-=\frac{1atm*5.0L}{0.082 \frac{atm*L}{mol*K} * 273.15K}*4\\Electricity=0.893Faraday$

Best regards.