Bond energy of `F_2` is 150 kJ `mol^(-1)`. Calculate the minimum frequency of photon to break this bond.

Calculate the energy required to excited one litre of hydrogen gas at 1 atm and 298 K to the excited state of atomic hydrogen. The energy for the disociation of H-H bond is 436 kJ mol^(-1) . Also calculate the minimum frequency of photon to break this bond.

Find the energy required to excite 1.10L od hydrogen gas at 1.0 nm and 298 K to the first excited state of atomic hydrogen .The energy required for the dissacitation of H-H bond is 436 kJ mol^(-1) .Also calculate the minimum frequency of a photon to break this bond

Bond dissociation on energy of Cl_(2) is 240 kJ/mol. The longest wavelength of photon that can break this bond would be [N_(A)=6xx10^(23), h=6.6xx10^(-34)J/s]

Bond dissociation on energy of Cl_(2) is 240 kJ/mol. The longest wavelength of photon that can break this bond would be [N_(A)=6xx10^(23), h=6.6xx10^(-34)J/s]

Bond energy of N-N is x kJ "mol"^(-1) . Then bond energy of N-=N is

If the bond energy of C-H bond is +416.18 kJ*mol^(-1) , then what will be the enthalpy of formation of C-H bond?

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 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)