If, when electrolyzing water (2H2O --> 2H2 + O2), the total bond energy of the reactants is 2000kJ and the total bond energy of the products is 934kJ, what is the total energy of the reaction and is this an endothermic or exothermic reaction?
Looks like you had to put in 2000 - 934 kJ so it is endothermic
You could have guessed that because when the Hindenberg burned H2 and O2 combined the other direction and heat was released.
I forgot the answer choices
1066kJ, exothermic
-1066kJ, exothermic
-1066kJ, endothermic
1066kJ, endothermic
the negative or positive one?
oh wait it would be the positive one
delta H reaction = (bond energy reactants - bond energy products)
Note that this is for gas reactions only.
To determine the total energy of the reaction and whether it is endothermic or exothermic, we need to compare the energy of the reactants with the energy of the products.
The reactants in this case are water molecules (2H2O), and the products are hydrogen gas (2H2) and oxygen gas (O2). The bond energy is the amount of energy required to break the bonds in the reactants and form the new bonds in the products.
Given that the total bond energy of the reactants is 2000 kJ and the total bond energy of the products is 934 kJ, we can calculate the energy change of the reaction.
The energy change (ΔE) of the reaction can be determined using the equation:
ΔE = Energy of products - Energy of reactants
ΔE = 934 kJ - 2000 kJ
ΔE = -1066 kJ
The negative value indicates that the energy of the products is lower than the energy of the reactants. This means that the reaction releases energy, making it an exothermic reaction.
Therefore, the total energy of the reaction is -1066 kJ and it is an exothermic reaction.