Enthalpy is the measurement of total energy change of a reaction.
The energy of bond formation and bond breaking can be used to calculate the bond enthalpy of the reaction. Bond enthalpy is the enthalphy change when 1 mol of bond is broken. Therefore the general equation to calculate the enthalpy change is energy of bond broken subtract by energy of bond formation.
Bond enthalpy is the energy required to break a chemical bond whereas lattice energy is the enthalpy of formation of one mole of an ionic compound from gaseus ions under standard conditions.
The enthalpy change associated with a reaction = sum of (energies of bonds broken) - sum of (energies of bonds formed). Thus, if this value is net negative, the reaction is exothermic; the products are also more stable than the reactants (lower-energy bonds). A positive enthalpy indicates an endothermic reaction.
Molar bond enthalpy shows the change in a bond association. For example, if one mole of bond is broken, the energy change that results is DHd (degree).
The bond forming process is always exothermic.
One mole of a particular bond is broken in the gas phase.
no
Bond enthalpy is the energy required to break a chemical bond whereas lattice energy is the enthalpy of formation of one mole of an ionic compound from gaseus ions under standard conditions.
Bond Dissociation Enthalpy is the energy required for breaking the bonds. This energy is supplied mostly by giving thermal energy (Heat).
the enthalpy of atomisation of hydrogen is equal and (in principle) identical to the bond dissociation enthalpy of the H-H bond. However, IF the first is measured by calorimetry and the second by spectrometry there might be a systematic difference.
positive
The enthalpy change associated with a reaction = sum of (energies of bonds broken) - sum of (energies of bonds formed). Thus, if this value is net negative, the reaction is exothermic; the products are also more stable than the reactants (lower-energy bonds). A positive enthalpy indicates an endothermic reaction.
Molar bond enthalpy shows the change in a bond association. For example, if one mole of bond is broken, the energy change that results is DHd (degree).
Look at the problem from the other angle why does it take energy to break up an ionic lattice. It is because of the electrostatic attrction of the ions which has to be overcome. A measure of the is energy is the lattice enthalpy which depends on the charges, th einterionic distances and the geometry of the lattice.
945.33 kJ/mol
Enzymes, as used in reactions, usually do not causes bond formation. They are usually responsible for breaking of bonds but when used in bond formation, they are commonly catalysts. Catalysts simply provide a lower activation energy and causes the reaction to occur faster. Thus, without catalysts, the reaction (including bond formation) will still occur, just at a slower rater. Thus, bond formation can definitely occur without enzymes (catalysts).
energy is released when the ATP hydrogen bond breaks, there are three hydrogen bonds by gabriela diaz
The bond forming process is always exothermic.