This reaction is not intense in cold water. When Mg metal is in contact withhot wateror steam, the bonds between its atoms break up which then causes the atoms to donate their electrons promptly. As hydrogen atoms do not tend to adsorb on thehot surfaceof Mg, the Mg metals are freely ...
And then it asked me to tell whether this reaction is endothermic or exothermic: H2+ Cl2---> 2 HCl I know that the bond enthalpy is calculated as Hreagents- Hproducts, but I'm still confused. Isn't the bond enthalpy the energy needed to break the bonds between the ions? Then how e...
BENDOMEX Where the energy from bond forming exceeds that needed for bond breaking the reaction is exothermic. Where the energy for bond breaking exceeds that from bond forming the reaction is endothermic. Energy in chemicals reactants products H Bonds break Bond forming Bonds form Exo Endo H...
and also the amount of the energy that is released when the bonds are formed. Consequently, if the bonds in your reactants have a higher total bond energy than your products, the reaction will be endothermic. If
* Endothermicandexothermicreactions Step1:EnergymustbeSUPPLIEDtobreakchemicalbonds: Step2:EnergyisRELEASEDwhennewchemicalbondsaremade: AreactionisEXOTHERMICifmoreenergyisRELEASEDthanSUPPLIED.IfmoreenergyisSUPPLIEDthanisRELEASEDthenthereactionisENDOTHERMIC ©Teachable.Somerightsreserved.http://teachable.net/res.asp?
Conversely, energy is required to break chemical bonds. Thus, reactions such as pyrolysis (discussed in Chapter 4) are endothermic. These important concepts are useful in understanding the chemistry of fire and its related reactions. Endothermic v. Exothermic Reactions A chemical reaction will either...