For a particular isomer of C8H18, the following reaction produces 5113.3 kJ of heat per mole...

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For a particular isomer of C8H18, the following reaction produces 5113.3 kJ of heat per mole...

For a particular isomer of C8H18, the following reaction produces 5113.3 kJ of heat per mole of C8H18(g) consumed, under standard conditions.

C8H18 + 25/2(O2) -> 8CO2 + 9H2O
DeltaH= -5113.3 kJ

What is the standard enthalpy of formation of this isomer of C8H18(g)?

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Answer 1

Answer #1

Concept and reason

The concept used is to calculate the enthalpy of formation of from the enthalpy change for the reaction and enthalpy of formation of other reactants/products.

Fundamentals

Enthalpy is the heat content of a system. Enthalpy changes for a reaction may be exothermic or endothermic.

The enthalpy change for the reaction is the amount of energy gained or lost during the reaction. It is represented as .

For a reaction, the enthalpy change is calculated as follows:

ΔΗ-Σ(ΔΗ,)ΔΗ,)

1.

The given reaction is as follows:

CH,8 (8)+25,02(g)
+8C02(g)+9H,0(8)
AHºrx = -5113.3 kJ/mol

The expression for the entropy change for the reaction is as follows:

ΔΗ, ° =[8ΔΗ, (Co,) + 9ΔΗ,°(Η,ο)]-[ΔΗ,°(CH) + 25% ΔΗ, (0,

AH, (H,0)=-241.8 kJ/mol
AH,(CO2) =-393.5 kJ/mol
AH, (02)=0 kJ/mol

The enthalpy for the reaction is calculated as follows:

-5113.3 kJ/mol = [8(-393.5)+9(-241.8) kJ/mol]-[AH,(CH))+252(0) kJ/mol]
-5113.3 kJ/mol = -5324.2 kJ/mol - AH,°(CH,x)
AH, (CH)=

Ans: Part 1

Therefore, the enthalpy of formation of is .

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Answer 2

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