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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?


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.

a. Endothermic

b. 678 kJ/mol

c. - 247 kJ/mol

d. Exothermic

e. 862 kJ/mol

f. + 1540 kJ/mol

g. +184 kJ/mol

h. True

i. 431 kJ/mol

j. False

1 How Much Energy Must Be Absorbed To Break The Bonds Of The 2 Molecules Of HCl2 How Much Energy Is Released When The Bonds Of H2 And Cl2 Form In The Products3 class=

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Bond energy refers to the energy that must be taken in to break a bond. It is also the energy required to form the bond.

What is Bond energy?

The term bond energy refers to the energy that must be taken in to break a bond. It is also the energy required to form the bond.

The energy that must be supplied to break the bonds in two molecules of HCl is 862 J. The energy released is obtained from; 862J - [436 +262] = 164J.

The total energy of the reaction is 164J, this is called the enthalpy change. Based on this value of the total energy, the reaction is endothermic. Hence, it is true that; "It takes more energy to break the two H–Cl bonds than is released when forming the H–H and Cl–Cl bonds."

Learn more about bond energy:https://brainly.com/question/16754172?

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