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. More bond energy is absorbed on the reactants side than is released on the products side.
B. The total bond energy of water and sodium chloride is greater than the total bond energy of hydrochloric acid and sodium hydroxide.
C. The energy of each bond in water and sodium chloride is greater than the energy of each bond in hydrochloric acid and sodium hydroxide.
D. 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.
2 answers
The answer is (B.) The total bond energy of water and sodium chloride is greater than the total bond energy of hydrochloric acid and sodium hydroxide
Let me point out that the question is flawed.
1. The reaction between HCl and NaOH is EXOTHERMIC by approximately 50 kJ/mol.
2. The use of bond energies to calculate delta H or to make conclusions based on delta H is valid ONLY for gases. These are not gases.
1. The reaction between HCl and NaOH is EXOTHERMIC by approximately 50 kJ/mol.
2. The use of bond energies to calculate delta H or to make conclusions based on delta H is valid ONLY for gases. These are not gases.
1 answer