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When 2 moles of C(2)H(6)(g) are complete...

When 2 moles of `C_(2)H_(6)(g)` are completely burnt `3120` kJ of heat is liberated. Calculate the enthyalpy of formation, of `C_(2)H_(6)(g)`. Given `Delta_(f)H` for `CO_(2)(g)` & `H_(2)O(l)` are `-395` & `-286` kJ respectively.

Text Solution

Verified by Experts

The correct Answer is:
`-88` kJ/mol
`{:(C_(2)H_(6)+7/2 O_(2) rarr 2CO_(2)+3H_(2)O,DeltaH=-1560,.........(1)),(C+O_(2) rarr CO_(2),DeltaH=-395,.........(2)),(H_(2)+1/2 O_(2) rarr H_(2)O,DeltaH=-286,.........(3)):}`
`rArr" "` Target reaction `2C+3H_(2) rarr C_(2)H_(6) " "DeltaH=?`
`DeltaH` can be obtained by `(2) xx2+(3)xx3-(1)`
`DeltaH=-88" kJ mol"^(-1)`
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Knowledge Check

  • The standard enthalpy of formation of octane (C_(8)H_(18)) is -250kJ //mol . Calculate the enthalpy of combustion of C_(8)H_(18) . The enthalpy of CO_(2)(g) and H_(2)O(l) are -394 kJ//mol and -286kJ//mol respectively.

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  • Heat of formation of benzene, CO_(2(g)) and H_(2)O_((l)) are 45 kJ, -394 kJ and - 286 kJ respectively. Hence heat of combustion of benzene is

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