If the bond enthalpy of `O_(2),N_(2)" and "H_(2)` are 498, 946 and 435.8 kJ `mol^(-1)` respectively. Choose the correct order of decreasing bond strength.

Calculate the bond enthalpy of H-CI given that the bond enthalpies of H_(2) and CI_(2) are 435.4 and 242.8 kJ "mol"^(-1) respectively and enthalpy of formation of HCI(g) is -92.2 kJ mol

The bond dissociatio of the molecules A_(2),B_(2),C_(2) are 498, 158, 945 kJ/mole respectively. If So, the correct decreasing order of their bond orders is

H_(2)(g) + (1)/(2)O_(2)(g) rarr H_(2)O(g) Delta H = -242 kJ mol^(-1) . Bond energy of H_(2) and O_(2) are 436 mol^(-1) and 500 mol^(-1) respectively. What is the bond energy of the O-H bond ?

The bond dissociation of the molecules A_2 , B_2,C_2 are 498, 158, 945 kJ/ mole respectively. If so, the correct decreasing order of their bond orders is

Bond dissociation enthalpies of H_(2(g)) and N_(2(g)) are "426.0 kJ mol"^(-1) and "941.8 kJ mol"^(-1) , respectively, and enthalpy of formation of NH_(3(g))" is "-"46 kJ mol"^(-1) . What are the enthalpy of atomisation of NH_(3(g)) and the average bond enthalpy of N-H bond respectively ( in kJ "mol"^(-1) )?

Bond dissociation enthalpies of H_(2(g)) and N_(2(g)) are "426.0 kJ mol"^(-1) and "941.8 kJ mol"^(-1) , respectively, and enthalpy of formation of NH_(3(g))" is "-"46 kJ mol"^(-1) . What are the enthalpy of atomisation of NH_(3(g)) and the average bond enthalpy of N-H bond respectively ( in kJ "mol"^(-1) )?

H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g) DeltaH =- 242 kJ mol^(-1) Bond energy of H_(2) and O_(2) is 436 and 500 kJ mol^(-1) , respectively. What is bond energy of O-H bond?

H_(2)(g) +(1)/(2)O_(2)(g) rarr H_(2)O(g) DeltaH =- 242 kJ mol^(-1) Bond energy of H_(2) and O_(2) is 436 and 500 kJ mol^(-1) , respectively. What is bond energy of O-H bond?