The combustion of a hydrocarbon is shown below:
C7H16(l) + 11O2(g) --> 7CO2(g) + 8H2O(g) ΔHcomb = -4822kj
If ΔHvap of water is 41kj/mol then what is the enthalpy of
combustion for one mole of this hydrocarbon if liquid water is a
product instead of water vapor?
The combustion of a hydrocarbon is shown below: C7H16(l) + 11O2(g) --> 7CO2(g) + 8H2O(g) ΔHcomb = -4822kj If ΔHvap of wa
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answerhappygod
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The combustion of a hydrocarbon is shown below: C7H16(l) + 11O2(g) --> 7CO2(g) + 8H2O(g) ΔHcomb = -4822kj If ΔHvap of wa
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