The volume of hydrogen gas (at STP) required each month to generate the electricity needed for a typical house is 5.107 * 10⁵ L
Redox reactions
Redox reactions are reactions in which oxidation and reduction occur simultaneously and to the same degree.
In a redox reaction, oxidation occurs at the anode while reduction occurs at the cathode.
Reactions occurring at the hydrogen-oxygen fuel cell
At the anode: 2 H₂ (g) + 4 OH⁻ (aq) ---> 4 H₂O + 4 e⁻
Oxidation potential, E°ox = 0.83 V
At the cathode: O₂ (g) + 2 H₂O (l) + 4 e⁻ ----> 4 OH⁻ (aq)
E°red = 0.40 V
Overall reaction: 2 H₂ (g) + -O₂ (g)--> 4 H₂O
E° = 1.23 V
Energy used in C.V
Energy used = 1500 kWh
I kWh = 3.6 * 10⁶ J = 3.6 * 10⁶ C.V
Then, energy used = 1500 * 3.6 * 10⁶ C.V
energy used = 5.4 * 10⁹ C.V
Charge carried on electrons
Charge carried by electrons = Energy/voltage
Total charge carried = 5.4 * 10⁹ C.V/1.23
Charge on electrons = 4.39 * 10⁹ C
Calculating moles of electrons
1 e = 96500 C
Number of electrons that carries a charge of 4.39 * 10⁹ C = 4.39 * 10⁹ C/96500 C
Number of electrons = 4.55 * 10⁴ mole of electrons
From the equation of reaction, 2 moles of H₂ produces 4 moles of electrons
Moles of hydrogen that produces 4.55 * 10⁴ = 4.55 * 10⁴/2
Moles of hydrogen that produces 4.55 * 10⁴ = 2.28 * 10⁴ moles
I mole of hydrogen = 22.4 L
2.28 * 10⁴ moles of hydrogen gas has a volume = 2.28 * 10⁴ * 22.4
2.28 * 10⁴ moles of hydrogen gas has a volume of 5.107 * 10⁵ L
Therefore, the volume of hydrogen gas (at STP) required each month to generate the electricity needed for a typical house is 5.107 * 10⁵ L
:Learn more about fuel-cell generators at: https://brainly.com/question/1220513
