Home
Class 12
CHEMISTRY
Calculate the bond energy of C - H bond...

Calculate the bond energy of `C - H` bond, given that the heat of formation of `CH_4`, heat of sublimation of carbon and heat of dissociation of `H_2` are `-74.8 + 719.6 and 435 kJ mol^(-1)` respectively.

Text Solution

AI Generated Solution

To calculate the bond energy of the C-H bond in methane (CH₄), we will use the given thermodynamic data: the heat of formation of CH₄, the heat of sublimation of carbon, and the heat of dissociation of H₂. ### Step-by-Step Solution: 1. **Identify the Given Data:** - Heat of formation of CH₄ (ΔH_f) = -74.8 kJ/mol - Heat of sublimation of carbon (ΔH_sub) = 719.6 kJ/mol - Heat of dissociation of H₂ (ΔH_diss) = 435 kJ/mol ...
Promotional Banner

Similar Questions

Explore conceptually related problems

Calculate the resonance enegry of isoprene (C_(5)H_(8)) from the data given. Standard Heats of combustion of isoprene, carbon and hydrogen are -3186, -393.5 , and -285.83 kJ mol^(-1) , respectively. Bond energies of C=C, C-C, C-H and H-H bonds are 615, 348, 413 and 435.8 kJ mol^(-1) respectively. Standard heat of sulbilmation of graphite is 718.3 kJ mol^(-1) .

If the heat of formation of MH_(4) is -1600 kJ, the bond energy of M-H would be :

Calculate the enthalpy of formation of water, given that the bond energies of H-H, O=O and O-H bond are 433 kJ mol^(-1), 492 kJ mol^(-1) , and 464 kJ mol^(-1) , respectively.

Calculate the heat of formation of Benzene. The reaction is given below - 6C(s)+3H_(2)rarr C_(6)H_(6)(l) and - 3268, - 393.5 nd -285.8 kJ are the heat of combustion of Benzene, heat of formation of CO_(2) and heat of formation of H_(2)O(l) respectively.