The enthalpy change for the process C_(("graphite")) rarr C(g), Delta H = +x KJ represents enthalpy of
The enthalpy of the reaction H _(2 (g)) + 1/2 O _(2(g)) to H _(2) O _((g)) is Delta H _(1) and that of H _(2(g)) + 1/2 O _(2(g)) to H _(2) O _((l)) is Delta H _(2). Then
Calculate the standard internal change in multiples of -10^(2)KJ for the reaction OF_(2(g)) + H_(2)O_((g)) rarr O_(2(g)) + 2HF_((g)) at 298K. The standard enthalpies of formation of OF_(2(g)), H_(2)O_((g)), HF_((g)) " are " +20, -250 and -270KJ "mole"^(-1)
What is the bond enthalpy of C-H bond of CH_(4) ?
For the reaction: 2H_(2(g)) + O_(2(g)) rarr 2H_2O_((g)) , DeltaH = -571 kJ bond energy of (H-H) = 435 kJ, of (O = O) = 498kJ , then the average bond energy of O-H bond using the above data
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:
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column