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Given C(2)H(2)(g)+H(2)(g)rarrC(2)H(4)(g)...

Given `C_(2)H_(2)(g)+H_(2)(g)rarrC_(2)H_(4)(g): DeltaH^(@)=-175 " kJ mol"^(-1)`
`DeltaH_(f(C_(2)H_(4),g))^(@)=50 " kJ mol"^(-1), DeltaH_(f(H_(2)O,l))^(@)=-280 " kJ mol"^(-1), DeltaH_(f(CO_(2)g))^(@)=-390 " kJ mol"^(-1)`
If `DeltaH^(@)` is enthalpy of combustion (in kJ `"mol"^(-1)`) of `C_(2)H_(2)`(g), then calculate the value of `|(DeltaH^(@))/(257)|`

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Knowledge Check

  • If DeltaH_(f(C_(2)H_(6)))^(0)(g) = -85 KJH mol^(-1) , DeltaH_(f(C_(3)H_(8)))^(0) (g) = -104 KJ mol^(-1), DeltaH^(0) for C (s) rarr C(g) is 718 KJ mol^(-1) and heat of formation of H-atom is 218 KJmol^(-1) then :

    A
    `DeltaH_(C-C) = 345` KJ
    B
    `DeltaH_(C-H) = 414` KJ
    C
    `DeltaH_(H-H)=436 KJ`
    D
    `DeltaH_(H-H) = 436` KJ

  • For the reaction 3N_(2)O(g)+2NH_(3)(g)to4N_(2)(g)+3H_(2)O(g),DeltaH^(@)=-879.6kJ If DeltaH_(f)^(@)[NH_(3)(g)]=-45.9kJ" "mol^(-1) , DeltaH_(f)^(@)[H_(2)O(g)]=-241.8kJ" "mol^(-1) Then DeltaH_(f)^(@)[N_(2)O(g)] will be:

    A
    `+246` kJ
    B
    `+82` kJ
    C
    `-82kJ`
    D
    `-246kJ`

  • In the reaction CO_(2)(g)+H_(2)(g)rarrCO(g)+H_(2)O(g), DeltaH=2.8 kJ DeltaH represents

    A
    Heat of reaction
    B
    Heat of combustion
    C
    Heat of formation
    D
    Heat of solution

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