378 π 965 weaker o 265 Using the data here, the difference in energy between a carbon-carbon double bond and a carbon- carbon single bond is kJ/mol. This value represents the energy of a bond. From this data, a π bond is than a o bond. However, numerous other sources list the average carbon-carbon double bond energy as approximately 615 kJ/mol. This would lead to the difference in energy between a carbon-carbon double bond and a carbon-carbon single bond of kJ/mol. From this data, a π bond is than a σ bond.

Calculate the ΔHrxn using bond enthalpies for the balanced equation below (Lewis structures also provided).   Bond Enthalpy Values: Bond ΔH (kJ/mol) C=C 611 C–H 414 H–H 436 C–C 347 Group of answer choices -219 kJ -128 kJ 286 kJ -564 kJ

Is this system endothermic or exothermic, and why? * H2 + CO2 CH202 Reactant bond energies: H-H is 432 kJ/mol, C=O is 799 kJ/mol Product bond energies: C-H is 413 kJ/mol, C=0 is 745 kJ/mol, C-O is 358 kJ/mol, O-H is 467 kJ/mol It is exothermic because more energy is given off by the products versus the amount needed to break up the reactants. It is exothermic because more energy is needed to break up the reactants versus the amount given off by the products. It is endothermic because more energy is needed to break up the reactants versus the amount given off by the products. It is endothermic because more energy is given off by the products versus the amount needed to break up the reactants.

If the following reaction is given: C2H5F + Cl2 || AHran If the bond energy for C-H is 414 kJ/ mole, the bond energy for C-C is 347 kJ/mole, the bond energy for C-Cl is 377 kJ/ mole, the bond energy for Cl-Cl is 243 kJ/ mole, the bond energy for C-F is 450 kJ/ mole and the done energy for H-Cl is 431 kJ/ mole, determine the bond energy for the H-F bond in kJ/mole. C2H4Cl2 + HF 151kJ mole Give your answer as a positive value as all energies for bond values should be written in terms of a positive value (the energy needed to break the bond = endothermic)