Calculate the enthalpy change for the process
`C CI_(4)(g)rarrC(g)+4CI(g)`
and calculate bond enthalpy of C - Cl in `C CI_(4)(g).`
`Delta_("vap")H^(Ө)(C CI_(4))=" " 30.5 kJ mol^(-1)`
`Delta_(f)H^(Ө)(C CI_(4))=-135.5kJ mol^(-1)`
`Delta_(a)(C)=715.0kJ mol^(-1)`, where `Delta_(a)H^(Ө)` is enthalpy of atomisation
`Delta_(a)H^(Ө)(CI_(2))=242 kJ mol^(-1)`

Calculate the enthalpy change for the process C Cl_(4)(g) rarr C(g)+4Cl(g) and calculate bond enthalpy of C-Cl in C Cl_(4)(g) . Delta_(vap)H^(Θ)(C Cl_(4))=30.5 kJ mol^(-1) Delta_(f)H^(Θ)(C Cl_(4))=-135.5 kJ mol^(-1) Delta_(a)H^(Θ)(C )=715.0 kJ mol^(-1) , where Delta_(a)H^(Θ) is enthalpy of atomisation Delta_(a)H^(Θ)(Cl_(2))=242 kJ mol^(-1)

Calculate P-Cl bond enthalpy P(s)+(3)/(2)Cl_(2)(g)rarr PCl_(3)(g) Given : Delta_(f)H(PCl_(3),g)=306kJ //mol DeltaH_("atomization")(P,s)=314kJ//mol , Delta_(r)H(Cl,g)=1231kJ//mol

Determine C-C and C-H bond enthalpy (in kJ//mol ) Given : Delta_(f)H^(@)(C_(2)H_(6),g)=-85kJ//mol," "Delta_(f)H^(@)(C_(3)H_(8),g)=-104kJ//mol Delta_("sub")H^(@)(C,s)=718kJ//mol," "B.E.(H-H)=436kJ//mol

Calculate the resonance energy of toluene (use Kekule structure from the following data C_(7)H_(8)(l) +9O_(2)(g) rarr 7CO_(2)(g) +4H_(2)O(l)+ DeltaH, DeltaH^(Theta) =- 3910 kJ mol^(-1) C_(7)H_(8)(l) rarr C_(7)H_(8)(g), DeltaH^(Theta) = 38.1 kJ mol^(-1) Delta_(f)H^(Theta) (water) =- 285.8 kJ mol^(-1) Delta_(f)H^(Theta) [CO_(2)(g)] =- 393.5 kJ mol^(-1) Heat of atomisation of H_(2)(g) = 436.0 kJ mol^(-1) Heat of sublimation of C(g) = 715.0 kJ mol^(-1) Bond energies of C-H, C-C , and C=C are 413.0, 345.6 , and 610.0 kJ mol^(-1) .

the bond enthalpy of H_(2)(g) is 436 kJ "mol"^(-1) and that of N_(2)(g) is 941.3 kJ"mol"^(-1) . Calculate the average bond enthalpy of ann N-H bond in ammonia, Delta_(t)^(@)(NH_(3)) =-46 kJ "mol"^(-1)

The enthalpy of atomisation for the reaction CH_(4) (g) rarr C (g) + 4H (g) " is " 1665 kJ mol^(-1) . What is the bond energy of C - H bond ?

Calculate DeltaH^(@) ("in" kJmol^(-1)) for the reaction CH_(2)Cl_(2)(g)rarrC(g)+2H(g)+2Cl(g). The average bond enthalpie of C-H and C-C1 bonds are 414 kJ mol^(-1) .

Determine the enthalpy change for the given reaction. CH_(4) (g) + Cl_(2) (g) rightarrow CH_(3) Cl(g) + HCI (g) Bond energies are given as follows: C-H = 412 kJ mol^(-1) C-CI = 338 kJ mol^(-1) CI-CI = 242 kJ mol^(-1) H-CI = 431 kJ mol^(-1) .

Calculate the lattice energy of the reaction Li^(o+)(g) +CI^(Theta) (g) rarr LiCI(s) from the following data: Delta_("sub")H^(Theta)(Li) = 160.67 kJ mol^(-1), (1)/(2)D(CI_(2)) = 122.17 kJ mol^(-1) IP(Li) = 520.07 kJ mol^(-1),E_(A)(CI) = - 365.26 kJ mol^(-1) and Delta_(f)H^(Theta)(LiCI) =- 401.66 kJ mol^(-1)

Find DeltaH of the process NaOH(s) rarr NaOH(g) Given: Delta_(diss)H^(Theta)of O_(2) = 151 kJ mol^(-1) Delta_(diss)H^(Theta) of H_(2) = 435 kJ mol^(-1) Delta_(diss)H^(Theta) of O-H = 465 kJ mol^(-1) Delta_(diss)H^(Theta) of Na -O = 255 kJ mol^(-1) Delta_(soln)H^(Theta)of NaOH = - 46 kJ mol^(-1) Delta_(f)H^(Theta) of NaOH(s) =- 427 kJ mol^(-1) Delta_("sub")H^(Theta) of Na(s) = 109 kJ mol^(-1)