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wel
3 years ago
9

If hydrogen were used as a fuel, it could be burned according to the following reaction: H2(g)+1/2O2(g)→H2O(g). Use average bond

energies to calculate ΔHrxn for this reaction Use average bond energies to calculate ΔHrxn for the combustion of methane (CH4). Which fuel yields more energy per mole and per gram?
Chemistry
1 answer:
serious [3.7K]3 years ago
7 0
The deltaHrxn = -243 kJ/mol the deltaHrxn of CH4(methane) = -802 kJ/mol 

The fuel that yields more energy per mole is METHANE. The negative sign merely signifies the release of energy. Thus, 802 kJ/mol is greater than 243 kJ/mol.

The fuel that yields more energy per gram is HYDROGEN. Here is the computation:
deltaHrxn = (-243 kJ/mol)(1 mol/2.016 g H2)  <span>= -120.535714286 kJ/g or -121 kJ/g

</span>deltaHrxn of CH4(methane) = (-802 kJ/mol)(1 mol/16.04 g) 
<span>= -50 kJ/g 
</span>
As discussed the negative sign serves as the symbol of released energy. Thus, 121 is greater than 50.
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in the problem the product formed after radiation was Pb-206. isotopes of lead include Pb-204, Pb-206, Pb-207, Pb-208. they all have atomic number 82. which means the radiation cannot be ∝ or β since both radiations will alter the atomic number of the parent nucleus.

Only gamma radiation with \left \{ {{y=0} \atop {x=0}}γ \right. will produce a Pb-206 of atomic number 82 and mass number 206 , since gamma ray have 0 mass and has 0 atomic number.equation is shown below

\left \{ {{y=206} \atop {x=82}}Pb\right ⇒ \left \{ {{y=206} \atop {x=82}}Pb\right +  \left \{ {{y=0} \atop {x=0}}γ\right.

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