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Gasoline is a mixture of hydrocarbons, but the heat released when it burns is close to that of octane, C₈H₁₈(l) ( ΔHf° = -250.1 kJ/mol). Research is underway to use H₂ from the electrolysis of water in fuel cells to power cars instead of gasoline.(b) How many liters of H2 at 25°C and 1.00 atm must burn to produce this quantity of energy?

Respuesta :

11,961 L volume of H2 at 25°C and 1.00 atm must burn to produce -118, 167kJ quantity of energy.

Chemical equation

H2 (g) + ½ O2 (g) » H2 O (g)

Calculation of the heat of reaction

∆H° rxn = (∆H° (H2O) ) – (∆H°(H2(g)) + ½ ∆H ° (O2(g))

= (-241.826 kJ / mol) – (0 kJ /mol + ½ ( 0 KJ /mol)

= -241. 826 kJ / mol

Number of moles of H2 can be calculated as

= -118167 KJ / -241. 826 KJ / mol

= 488.644 KJ /mol

Calculation of the volume

As we know that,

PV = nRT

where, P is the pressure

V is the volume of the gas

T is the temperature

n is the number of moles of gas

R is the gas constant

Volume = nRT / P

By substituting all the values, we get

= 488.644 mol × atm /mol × ( 25°C + 273.15 ) K / 1.0 atm

= 11.961 l

Therefore, the volume of the H2 is 11.961 L

Thus, we calculated that 11,961 L volume of H2 at 25°C and 1.00 atm must burn to produce -118, 167kJ quantity of energy.

learn more about ideal gas equation:

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