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

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:

For the reaction: 2H_(2(g)) + O_(2(g)) rarr 2H_2O_((g)) , DeltaH = -571 kJ bond energy of (H-H) = 435 kJ, of (O = O) = 498kJ , then the average bond energy of O-H bond using the above data

If the enthalpy change for the reaction CH_4(g)+Cl_2(g)rarrCH_3Cl(g)+HCl(g) , triangleH =-25 kcal. Bond energy of C-H is 20kcal/mol greater than the bond energy of C-Cl and bond energies of H-H and H-Cl are same in magnitude, then for the reaction: 1//2H_2(g)+1//2Cl_2(g)rarrHCl(g) triangleH is

Calculate Delta G (in kJ) for the reaction at 300 K, H_(2)(g)+Cl_(2)(g) rarr 2HCl (g) Given at 300 K, BE_(H-H) = 435 kJ mol^(-1), BE_(Cl-Cl) = 240 kJ mol^(-1), BE_(HCl) = 430 kJ mol^(-1) Entropies of H_(2), Cl_(2) and HCl are 131, 223 and 187 JK^(-1) mol^(-1) respectively.

In the reaction, H_2 + Cl_2 rarr 2HCl DeltaH =-184 kJ, if 2 moles of H2 react with 2 moles of Cl_2 , then DeltaU is equal to

H_(2) +Cl_(2) rarr 2HCl" "Delta H =-184 kJ Delta H" for "36.5 xx 10^(-2) kg is