Use the following table and chemical reaction to answer the questions #8 and #9.

Question

Use the following table and chemical reaction to answer the questions #8 and #9. Table A shows bond energies-the amount of energy required to break a chemical bond, and also the amount of energy released when a bond is formed. Use these bond energies to determine whether the following chemical reactions are exothermic or endothermic. (see information above) What is the net energy change of this reaction? a. 183 kj/mol b. 679 kj/mol c. 862 kj/mol d. 1541 kj/mol e e none of the above...the correct answer is _________ Kj/mol and all of my work to solve the problem is shown below. (see information above) The above chemical reaction can be classified (in an energy sense) as a. endothermic b. exothermic c. "balanced" in an energy sense...so neither endothermic nor exothermic. d. energetic e. Cannot be determined.

Explanation / Answer

1. Answer is Option A, 183 kj/mol

The net energy change of the reaction is obtained by calculating the sum of energis of products and reactants and finding the difference between them

Here the total energy of reactants = 436 + 243 = 679 kj/mol

total energy of products = 431 + 431 = 862 kj/mol

Net energy change = Energy of reactants - Energy of products

= 679-862 = -183kj/mol

The minus indicates the reaction is exothermic reaction.

2. Answer is Option B, Exothermic

Exothermic reaction is the reaction or process which releases heat. That means energy of products should be greater than the energy of the reactants. Here in theis case energy of products is 862kj/mol and energy of reactants is 679kj/mol suggesting that the reaction is exothermic.

Related Questions

Navigate

• Browse (All)
• Browse U
• Subjects

---

---

Integrity-first tutoring: explanations and feedback only — we do not complete graded work. Learn more.