For a particular isomer of C8H18, the combustion reaction produces 5104.1 kJ of heat per mole...

For a particular isomer of C8H18, the combustion reaction produces 5104.1 kJ of heat per mole of C8H18(g)

consumed, under standard conditions.

C8H18(g)+252O2(g)⟶8CO2(g)+9H2O(g)Δ?∘rxn=−5104.1 kJ/mol

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

Solutions

Expert Solution

Given:

ΔHo rxn = -5104.1 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) + 25/2 O2(g) ---> 8 CO2(g) + 9 H2O(g)

ΔHo rxn = 8*Hof(CO2(g)) + 9*Hof(H2O(g)) - 1*Hof( C8H18(g)) - 25/2*Hof(O2(g))

-5104.1 = 8*(-393.509) + 9*(-241.818) - 1*Hof(C8H18(g)) - 25/2*(0.0)

Hof(C8H18(g)) = -220.334 KJ/mol

Answer: -220.334 KJ/mol

queen_honey_blossom answered 1 year ago

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