Hydrochloric acid and sodium hydroxide react to produce water and sodium chloride in an endothermic reaction. Which statement must be true of the reaction?
A.The total bond energy of water and sodium chloride is greater than the total bond energy of hydrochloric acid and sodium hydroxide.
B.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.
C.More bond energy is absorbed on the reactants side than is released on the products side.**
D.The energy of each bond in water and sodium chloride is greater than the energy of each bond in hydrochloric acid and sodium hydroxide.
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The correct answer is C. More bond energy is absorbed on the reactants side than is released on the products side.
In an endothermic reaction, energy is absorbed from the surroundings, causing the reaction to feel cold. The reactants, hydrochloric acid (HCl) and sodium hydroxide (NaOH), have stronger bonds compared to the products, water (H2O) and sodium chloride (NaCl). Bond energy is the amount of energy required to break a bond.
To determine which statement is true, we need to compare the bond energies involved in the reaction. Since the reaction is endothermic (absorbs energy), it means that more energy is required to break the bonds in HCl and NaOH than is released when the bonds are formed in H2O and NaCl.
Therefore, the correct answer is C. More bond energy is absorbed on the reactants side than is released on the products side.