Heat evolved in the reaction `H_(2)+CL_(2)rarr2HCl` is `182KJ` . Bond energies of `H-H` and `Cl-Cl` are `430` and `242KJ//mol` resoectively. The `H-Cl` bond energy is

Heat evolved in the reaction, H_2+Cl_2rarr2HCl is 182 kJ. Bond energies of H-H and Cl-Cl are 430 and 242 kJ/mol respectively. The H-Cl bond energy is

Heat evolved in the reaction, H_2+Cl_2rarr2HCl is 182 kJ. Bond energies of H-H and Cl-Cl are 430 and 242 kJ/mol respectively. The H-Cl bond energy is:

Heat evolved in the reaction H_(2)+Cl_(2) rarr 2HCl is 182 kJ Bond energies H- H = 430 kJ/mole, Cl-Cl = 242kJ//"mole" . The H-Cl bond energy is

Heat evolved in the reaction H_(2)[g]+Cl_(2)[g] rarr 2HCl[g] is 182 kJ Bond energies H- H = 430 kJ/mole, Cl-Cl = 242kJ//"mole" . The H-Cl bond energy is

Calculate free energy change at 27^(@)C for the reaction H _(2) + Cl _(2) to 2 HCl Given bond enthalpies of H_(2), Cl_(2) and HCl are 435, 240 and 430 kJ mol^(-1) respectively and entropies of H_(2), Cl_(2) and HCl are 131,223 and 187 JK^(-1) respectively

What will be DeltaH for the reaction, CH_(2)Cl_(2)rarrC+2H+2Cl ? (B.E. of C-H and C-Cl bonds are "416 kJ mol"^(-1) and "325 kJ mol"^(-1) respectively)

Find Delta_(f)H of HCl (g) if bond energies of H_(2), Cl_(2) and HCl are 104, 58, 103 kcal/mol respectively.

Find Delta_(f)H of HCl (g) if bond energies of H_(2), Cl_(2) and HCl are 104, 58, 103 kcal/mol respectively.