1. How much energy must be absorbed to break the bonds of the 2 molecules of HCl?

Question

2. How much energy is released when the bonds of H2 and Cl2 form in the products?

3. What is the total energy of the reaction? (Use the formula: Total bond energies of reactants - Total bond energies of products)

4. Based on the value of the total energy of the reaction, is this reaction endothermic or exothermic?

5. True or False - It takes more energy to break the two H–Cl bonds than is released when forming the H–H and Cl–Cl bonds.

2HCl(aq) --> H2(g) + Cl2(g)

H---Cl
------> H---H + Cl ----- Cl
H---Cl

Total bond energy for reaction = Total bond energy of reactants -- Total bond energy of products

bond Bond energy
H-Cl 431
H-H 436
Cl-Cl 242

Answer 1

I don't understand what your problem (what trouble you're having) solving this. You have the bond energies listed, you have the correct formulas. Clue me in.

Answer 2

You're right, I tried harder to do it myself instead of asking for help and succeeded, thank you for the motivation lol

Answer 3

So what did you get?

Answer 4

@ Am dumm faxx help me check my work

Answer 5

What are the answers?