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The bond dissociation energy depends upo...

The bond dissociation energy depends upon the nature of the bond and nature of the molecule. If any molecule more than 1 bonds of similar nature are present then the bond energy reported is the average bond energy.
Heat evolved when 0.75 mol of molten aluminium at its melting point of `658^(@)C` is solidified and cooled to `25^(@)C`. The enthalpy of fusion of aluminium is `76.8 "cal" g^(-1) and C_(P)= 5.8 "cal" mol^(-1) ""^(0)C`

A

`-4.3` kcal

B

4.3 kcal

C

`-1.199k` cal

D

1.199kcal

Text Solution

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The correct Answer is:
A
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The highest bond energy is for

The bond dissociation energy depends upon the nature of the bond and nature of the molecule. If any molecule more than 1 bonds of similar nature are present then the bond energy reported is the average bond energy. Determine C-C and C-H bond enthalpy (in kJ/mol). Given: Delta_(f)H^(0) (C_(2)H_(6),g)= -85kJ//mol, Delta_(f) H^(0) (C_(3)H_(8), g)= -104kJ//mole, Delta_("sub")H^(0) (C,s)= 718kJ//mol , B.E. (H-H)= 436 kJ/mol,

Knowledge Check

  • The C-C bond dissociation energy is

    A
    103 K cals `"mole"^(-1)`
    B
    83 K cals `"mole"^(-1)`
    C
    8.3 K cals `"mole"^(-1)`
    D
    83 K cals `"mole"^(-1)`

  • The bond dissociation energy depends upon the nature of the bond and nature of the molecule. If any molecule more than 1 bonds of similar nature are present then the bond energy reported is the average bond energy. If enthalpy of hydrogenation of C_(6)H_(6(l)) "into" C_(6)H_(12(l)) " is " -205 kJ and resonance energy of C_(6)H_(6(l)) is -152kJ//mol then enthalpy of hydrogenation of is ? Answer Delta H_("vap") " of " C_(6)H_(6(l)), C_(6)H_(10(l)), C_(6)H_(12(l)) all are equal:

    A
    `-535.5kJ//mol`
    B
    `-238 kJ//mol`
    C
    `-357 kJ//mol`
    D
    `-119 kJ//mol`

  • The highest bond energy is for

    A
    `underset(sp)(C )-H`
    B
    `underset(sp^(2))(C )-H`
    C
    `underset(sp^(3))(C )-H`
    D
    All have equal energy

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