For a particular isomer of C8H18, the combustion reaction produces 5099.5 kJ of heat per mole...

Question

Question

For a particular isomer of C8H18, the combustion reaction produces 5099.5 kJ of heat per mole of C8H18(g) consumed, under standard conditions.

C8H18(g)+252O2(g)⟶8CO2(g)+9H2O(g)

Δ?∘rxn=−5099.5 kJ

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

Δ?∘f= kJ/mol

Answer 1

Answer #1

Given:

ΔHo rxn = -5099.5 KJ/mol

Hof(O2(g)) = 0.0 KJ/mol

Hof(CO2(g)) = -393.509 KJ/mol

Hof(H2O(g)) = -241.818 KJ/mol

Balanced chemical equation is:

C8H18(g) + 25 O2(g) ---> 8 CO2(g) + 9 H2O(g)

ΔHo rxn = 8*Hof(CO2(g)) + 9*Hof(H2O(g)) - 1*Hof( C8H18(g)) - 25*Hof(O2(g))

-5099.5 = 8*(-393.509) + 9*(-241.818) - 1*Hof(C8H18(g)) - 25*(0.0)

Hof(C8H18(g)) = -224.934 KJ/mol

Answer: -224.9 KJ/mol

Answer 2

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