Home
Class 12
CHEMISTRY
The dissociation energy of CH(4)(g) is 3...

The dissociation energy of `CH_(4)(g)` is 360 kcal `mol^(-1)` and that of `C_(2)H_(6)(g) is 620 kcal mol^(-1)`. The C-C bond energy

A

170 kJ/mol

B

50 kJ/mol

C

80 kJ/mol

D

220 kJ/mol

Text Solution

Verified by Experts

Promotional Banner

Similar Questions

Explore conceptually related problems

The average energy required to break a P-P bond in P_(4)(s) into gaseous atoms is 53.2 kcal mol^(-1) . The bond dissociation energy of H_(2)(g) is 104.2kcal mol^(-1) , Delta H_(f)^(0) of PH_(3)(g) from P_(4)(s) is 5.5 kcal mol^(-1) . The P-H bond energy in kcal mol^(-1) is [ Neglect presence of Van der Waals force in P_(4)(s) ]

The enthalpy of formation of UF(g) is 22kcal mol^(-1) and that of U(g) is 128kcal mol^(-1) . The bond energy of the F-F bond is 37kcal mol^(-1) . The bond dissociation energy of UF(g) is (are):

Find the electron affinity of chlorine from the following data. Enthalpy of formation of LiCI is -97.5 kcal mol^(-1) , lattice energy of LiCI =- 197.7 kcal mol^(-1) . Dissociation energy of chlirine is 57.6 kcal mol^(-1) , sublimation enthalpy of lithium =+ 38.3 kcal mol^(-1) , ionisation energy of lithium =123.8 kcal mol^(-1) .

An exothermic reaction, A rarr B , has an activation energy of "15 kcal mol"^(-1) and the energy of reaction is "5 kcal mol"^(-1) . The activation energy in "kcal mol"^(-1) for the reaction, BrarrA is

The lattice enthalpy of KI will be, if the enthalpy of (I) Delta_f H^- (KI) = -78.0 kcal mol^-1 (II) Ionisation energy of K to K^+ is 4.0 eV (III) Dissociation energy of I_2 is 28.0 kcal mol^-1 (IV) Sublimation energy of K is 20.0 kcal mol^-1 (V) Electron gain enthalpy for I to I^- is -70.0 kcal mol^-1 (VI) Sublimation energy of I_2 is 14.0 kcal mol^-1 (1 eV =23. 0 kcal mol^-1)

Given that CH_(4)(g) +360 kJ rarr C(g) +4H(g) C_(2)H_(6)(g) +620 kJ rarr 2C(g) +6H(g) The value of C-C bond enegry is

Calculate Delta_(f)H^(Theta) ICI(g) from the data DeltaH dissociation CI_(2)(g) = 57.9 kcal mol^(-1) DeltaH dissociation I_(2)(g) = 36.1 kcal mol^(-1) DeltaH dissociation ICI(g) = 50.5 kcal mol^(-1) DeltaH sublimation I_(2)(g) = 15.0 kcal mol^(-1)

Enthalpy of atomization of C_(2)H_(6)(g) and C_(3)H_(8)(g) are 620 and 880kJmol^(-1) respectively. The C-C and C-H bond energies are respectively

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) .

From the following data, calculate the standard enthalpy of formation of propane Delta_(f)H^(Theta) CH_(4) = - 17 kcal mol^(-1) Delta_(f)H^(Theta)C_(2)H_(6) =- 24 kcal mol^(-1), BE (C-H) = 99 kcal mol^(-1) (C- C) = 84 kcal mol^(-1) .