What is required, in terms of bond energies of reactants and products, for a reaction to be exothermic?(1 point)
Responses
The energy released in the formation of the reactants must be greater than the energy absorbed by the products.
The energy released in the formation of the products is the same as the energy absorbed by the reactants.
The energy released in the formation of the products must be greater than the energy absorbed by the reactants.
Bond energies do not influence chemical reactions.
The energy released in the formation of the reactants must be greater than the energy absorbed by the products.
aRE YOU SURE
I apologize for any confusion. The correct statement is:
The energy released in the formation of the products must be greater than the energy absorbed by the reactants.
which one is it
I apologize for the confusion. The correct statement is:
The energy released in the formation of the products must be greater than the energy absorbed by the reactants for a reaction to be exothermic.
The energy released in the formation of the products must be greater than the energy absorbed by the reactants.
The correct answer is:
The energy released in the formation of the reactants must be greater than the energy absorbed by the products.
To explain why, let's consider the concept of bond energies. Bond energies are the amount of energy required to break a specific bond between two atoms in a molecule, or the amount of energy released when a bond is formed. In a chemical reaction, new bonds are formed and existing bonds are broken.
In an exothermic reaction, energy is released to the surroundings, resulting in an overall decrease in the energy of the reacting system. This means that the energy released in the formation of the products is greater than the energy absorbed by the reactants.
When bonds are formed, energy is released because the atoms in the newly formed molecule are in a more stable state than as separate atoms. In contrast, when bonds are broken, energy is absorbed because the molecules are becoming less stable by losing their existing bonds.
Therefore, for a reaction to be exothermic, the energy released in the formation of the reactants must be greater than the energy absorbed by the products. This ensures that the reaction releases more energy than it absorbs, resulting in a net release of energy.