Coulombs needed to produce 3.53 × 10⁶ L of H₂ gas at 12.0 atm and 258°C is 3.31 × 10¹¹ C.
(a) The reaction is
2H₂O + 2e⁻ → H₂ + 2OH⁻
According to the reaction, 2 moles of electrons flow per mole of reaction,
(b) Given
T = 25°C = (25 + 273 ) K
= 298 K
F = 96500 C
We know that ,
PV =nRT
Hence ,
n = [tex]\frac{PV}{RT}[/tex]
= [tex]\frac{(12) (3.5 .10^{6}) }{(0.082057)(298)}[/tex]
= 1.7176 ×10⁶ mole
Now,
From the given reaction we can say that ,1 mole of H₂ is produced by 2 moles of electron
Hence, 1.7176 ×10⁶ mole of H₂ is produced by
= 2× 1.7176×10⁶ moles of electron
= 3.435 ×10⁶ moles of electron
We know that
charge = moles of electron × F
= (3.435 ×10⁶ × 96500) C
= 3.31 × 10¹¹ C
Thus from the above conclusion we can say that Coulombs needed to produce 3.53 × 10⁶ L of H₂ gas at 12.0 atm and 258°C is 3.31 × 10¹¹ C.
Learn more about Fuel Cell here : https://brainly.com/question/16612142
#SPJ4
Disclaimer : The question given was incomplete on portal, Here is the complete question.
Question : Car manufacturers are developing engines that use H₂ as fuel. In Iceland, Sweden, and other parts of Scandinavia countries, where hydroelectric plants produce inexpensive electric power, the H₂ can be made industrially by the electrolysis of water.
a) How many moles of electrons flow per mole of reaction ?
b) How many coulombs are needed to produce 3.53X10⁶ L of H₂ gas at 12.0 atm and 25°C.
