Hydrochloric acid and sodium hydroxide react to produce water and sodium chloride in an endothermic reaction. Which statement must be true of the reaction?(1 point) Responses The energy of each bond in water and sodium chloride is greater than the energy of each bond in hydrochloric acid and sodium hydroxide. The energy of each bond in water and sodium chloride is greater than the energy of each bond in hydrochloric acid and sodium hydroxide. The total bond energy of water and sodium chloride is greater than the total bond energy of hydrochloric acid and sodium hydroxide. The total bond energy of water and sodium chloride is greater than the total bond energy of hydrochloric acid and sodium hydroxide. More bond energy is absorbed on the reactants side than is released on the products side. More bond energy is absorbed on the reactants side than is released on the products side. The bond energy used to break the bonds in hydrochloric acid and sodium hydroxide is less than the energy released to form the bonds in water and sodium chloride.
The total bond energy of water and sodium chloride is greater than the total bond energy of hydrochloric acid and sodium hydroxide.
thats wrong
I apologize for the incorrect answer. Let me correct it.
More bond energy is absorbed on the reactants side than is released on the products side. The bond energy used to break the bonds in hydrochloric acid and sodium hydroxide is less than the energy released to form the bonds in water and sodium chloride.
To determine which statement must be true of the reaction, let's analyze the endothermic reaction of hydrochloric acid (HCl) and sodium hydroxide (NaOH) to produce water (H2O) and sodium chloride (NaCl).
In an endothermic reaction, more energy is absorbed than is released. This means that the reactant side has a higher bond energy than the product side, indicating that bonds are being broken in the reactants and formed in the products.
Based on this, we can eliminate the following statements:
- "The energy of each bond in water and sodium chloride is greater than the energy of each bond in hydrochloric acid and sodium hydroxide." This statement focuses on individual bond energies rather than the total bond energy of the compounds involved.
- "More bond energy is absorbed on the reactants side than is released on the products side." This statement suggests a comparison of the bond energy absorbed and released, which might not be accurate without considering the specific values.
Now let's compare the remaining statements:
- "The total bond energy of water and sodium chloride is greater than the total bond energy of hydrochloric acid and sodium hydroxide." This statement considers the total bond energy of both the reactants and the products. Since it states that the bond energy of the products is greater, it aligns with the concept of endothermic reactions. However, this statement doesn't directly mention the bond energy used to break the bonds in the reactants.
- "The bond energy used to break the bonds in hydrochloric acid and sodium hydroxide is less than the energy released to form the bonds in water and sodium chloride." This statement explicitly refers to the bond energy used to break the bonds in the reactants, suggesting that it is less than the energy released during the formation of the products. This aligns with the fundamental concept of an endothermic reaction.
Therefore, the correct statement must be: "The bond energy used to break the bonds in hydrochloric acid and sodium hydroxide is less than the energy released to form the bonds in water and sodium chloride."