Respuesta :
The joules are produced when coulombs are supplied at 1.44 V is 3.94 × 10^11 J and mass of oil burned to yield 3.94 × 10^11 J is 9850000 kg.
Given,
Volume = 2.9 × 10^6
Pressure = 12 atm.
Temperature = 25°C = 298 K
We know the equation
PV = nRT
where,
P is the pressure
V is the Volume
n is the number of moles
R is the gas constant = 0.0821 L atm/mol K
T is the temperature
Calculation of number of moles of H2
n = PV/RT
By substituting the value in above equation, we get
= 12 × 2.9 × 10^6/(0.0821 × 298K)
= 1.422 × 10^6 moles of H2
Chemical reaction
2H(+) + 2e- ------ H2
Coulomb charge needed
1.422 × 10^6 moles of H2 × 2mol e- /1 mol H2)
= 2.844 × 10^6
As we know that,
one mole of electrons = 96500 C = 9.65 × 10^4 C
Now,
2.844 × 10^6 moles of electron can be given as
2.844 × 10^6 × 96500
= 2.74 × 10^11 C
b) Coulomb supplied at 1.44 V
Joules produced = 2.74 × 10^11 C × 1.44
= 3.94 × 10^11 J
c) Given,
Combustion of oil yield = 4.0X10⁴ kJ/kg,
Mass of oil which is burned to yield 3.94 × 10^11 J
= 3.94 × 10^11 J / 4.0X10⁴ kJ/kg
= 0.985 × 10^7
9850000 kg
Thus, we found that the joules are produced when coulombs are supplied at 1.44 V is 3.94 × 10^11 J and mass of oil burned to yield 3.94 × 10^11 J is 9850000 kg.
learn more about current:
https://brainly.com/question/16595375
#SPJ4
DISCLAIMER:
The above question is incomplete. The complete question can be given as
QUESTION
Car manufacturers are developing engines that use H₂ as fuel. In Iceland, Sweden, and other parts of Scandinavia, where hydroelectric plants produce inexpensive electric power, the H₂ can be made industrially by the electrolysis of water.
(a) How many coulomb are needed to produce 2.9 × 10^6 L of H2 at 12 atm and 25° C.
(b) If the coulombs are supplied at 1.44 V, how many joules are produced?
(c) If the combustion of oil yields 4.0X10⁴ kJ/kg, what mass of oil must be burned to yield the number of joules
