1. How much energy must be absorbed to break the bonds of the 2 molecules of HCl?
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
So what did you get?
You're right, I tried harder to do it myself instead of asking for help and succeeded, thank you for the motivation lol
@ Am dumm faxx help me check my work
What are the answers?
1. To determine the amount of energy required to break the bonds of the two molecules of HCl, we need to know the bond energy of the H-Cl bond. The bond energy of the H-Cl bond is 431 kJ/mol.
2. To calculate the energy released when the bonds of H2 and Cl2 form in the products, we need to know the bond energies of the H-H and Cl-Cl bonds. The bond energy of the H-H bond is 436 kJ/mol, and the bond energy of the Cl-Cl bond is 242 kJ/mol.
3. To find the total energy of the reaction, we can use the formula: Total bond energies of reactants - Total bond energies of products. In this case, the reactant is 2 molecules of HCl, and the products are H2 and Cl2.
Total bond energy for the reaction = (2 x bond energy of H-Cl) - (bond energy of H-H + bond energy of Cl-Cl)
= (2 x 431) - (436 + 242)
= 862 - 678
= 184 kJ/mol
Therefore, the total energy of the reaction is 184 kJ/mol.
4. Based on the value of the total energy of the reaction, we can determine whether the reaction is endothermic or exothermic. If the total energy is positive, it means more energy is absorbed (endothermic). If the total energy is negative, it means more energy is released (exothermic). In this case, the total energy of the reaction is 184 kJ/mol, which is positive. Therefore, this reaction is endothermic.
5. False. In this reaction, the bond energy required to break the two H-Cl bonds is 431 kJ/mol. The energy released when forming the H-H and Cl-Cl bonds is (436 + 242) kJ/mol. Since the energy required to break the H-Cl bonds (431 kJ/mol) is less than the energy released when forming the H-H and Cl-Cl bonds (678 kJ/mol), it takes less energy to break the two H-Cl bonds than is released when forming the H-H and Cl-Cl bonds.