If a reaction requires more energy to break the bonds in the reactants than the amount of energy released when new bonds are formed, what does this tell us?

In an exothermic reaction, which is greater: the energy released from forming new bonds, or the energy needed to break existing bonds?

In a chemical reaction, what term describes the energy released when new bonds are formed

Which of the following statements is true?Breaking bonds and making bonds are both endothermicBreaking bonds is endothermic, making bonds is exothermicBreaking bonds is exothermic, making bonds is endothermicBreaking bonds and making bonds are both exothermic2When calculating energy changes from bond energies, what is the first thing you should do?Calculate the bond energies of the reactantsSubtract the bond energies of the products from those of the reactantsBalance the equationCalculate the bond energies of the products3If a reaction requires more energy to break the bonds in the reactants than the amount of energy released when new bonds are formed, what does this tell us?It is exothermicThe product is a gasIt is endothermicThe reactant is a solid4Calculate the energy required to break the bonds in propane (C3H8) given the following bond energies: C-C = 347 kJ/mol; C-H = 413 kJ/mol.1520 kJ/mol3998 kJ/mol4345 kJ/mol760 kJ/mol

xplain, in terms of bond breaking and bond forming, why energy is released during this reactio

Breaking a chemical bond _____________ energy from the surroundings