`Delta_("sub")H=`………………..`+`………………. .

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,

For an ideal solution, Delta_(mix)V is ……….and Delta_(mix)H is ………. .

The expression Delta_("sub"1)H^(Theta) =Delta_(fus)H^(Theta) +Delta_(vap)H^(Theta) is true at al

Use the following data to calculate Delta_("lattice") H^(Θ) " for " NaBr. Delta_("Sub")H^(Θ) for sodium metal = 108.4 kJ mol^(-1) , ionisation enthalpy of sodium = 496 kJ mol^(-1) , electron gain enthalpy of bromine = -325 kJ mol^(-1) , bond dissociation enthalpy of bromine = 192 kJ mol^(-1), Delta_(f) H^(Θ) " for " NaBr(s) = - 360.1 kJ mol^(-1)

Delta H_("fusion") of a substance is 'x' and Delta H_("vap") is 'y', then Delta H_("sublimation") will be

Calculate Delta_(r)S_("sys")^(@) for the following reaction at 373 K: CO(g) + H_(2)O(g) to CO_(2)(g) + H_(2)(g) Delta_(r)H^(@) = -4.1 xx 10^(4) J, Delta_(r)S^(@)("unv") = 56 J//K

Calculate Delta_fH^(@) ("in" (kJ)/("mol")) for C_2H_6(g) , if Delta_cH^@ [C("graphite")] = –393.5 (kJ)/(mol) , Delta_c H^@ [(H_2)g]= –286 (kJ)/(mol) and Delta_cH^@ [C_2H_6(g)] = –1560 (kJ)/(mol)

If enthalpy of overall reaction XrarrY along one route is Delta_(r)H and Delta_(r)H_(1),Delta_(r)H_(2),Delta_(r)H_(3) …. Representing enthalpies of reactions leading to same product Y then Delta_(r)H is

Enthalpy is an extensive property. In general, if enthalpy of an overall reaction A rarr B along one route is Delta_(r) H " and Delta_(r) H_(1), Delta_(r) H_(2), Delta_(r) H_(3) ..... Represent enthalpies of intermediate reactions leading to product B. What will be the relation between Delta_(r)H overall reaction and Delta_(r)H_(1), Delta_(r)H_(2) ... etc for intermediate reaction.

A: Total enthalpy change of a multistep process is sum of Delta H_(1) + Delta H_(2) + Delta H_(3) + .... R: When heat is absorbed by the system, the sign of q is taken to be negative.