Given that the average bond enthalpies, estimate the enthalpy of atomisation for the following diborane (H2B-BH2)

The compound diborane (B2H6) is used as a rocket fuel. The equation for the combustion of diborane is shown below.B2H6 (g) + 3O2 (g) → B2O3 (s) + 3H2O(l)Calculate the enthalpy of combustion of diborane (B2H6) in kJ mol−1 to 1 d.p, using the following data.2B(s) + 3H2(g) → B2H6 (g) ΔH = 40.29 kJ mol−1H2(g) + ½O2(g) → H2O(l) ΔH = −286 kJ mol−12B(s) + 1½O2(g) → B2O3(s) ΔH = −1274 kJ mol−1

Given the following bond dissociation energies, calculated the enthalpy of the following reaction.CH4 + 2F2 → CF4 + 2H2Hint: You might need to draw Lewis Dot Structures for each of these before you can count the bonds on the reactant and product sides.C-F            450 kJ/molC-H            410 kJ/molF-F            158 kJ/molH-H            436 kJ/molGroup of answer choices318 kJ-716 kJ-318 kJ716 kJ

Given the following bond dissociation energies, calculated the enthalpy of the following reaction.H-C≡C-H + 2H2 → H3C-CH3C-C            350 kJ/molC≡C           807 kJ/molC-H            410 kJ/molH-H            436 kJ/molHint: There are 2 H-H bonds on the left and a total of 6 C-H bonds on the right.Group of answer choices-111 kJ/mol-211 kJ/mol-311 kJ/mol-11 kJ/mol

Which of the following correctly represents reaction for estimating standard enthalpy of formation of HBr?

Some lipids contains carbon to carbon double bonds.Given the bond dissociation energies in the table, calculate the enthalpy change when one mole of hydrogen is added across one double bond. A.+1520 kJ/molB.-1520 kJ/molC.+120 kJ/molD.-120 kJ/mol