Question

During an endothermic reaction, H for the reactants was −600 kJ/mol. Which of the following statements is correct about the H for the products and the comparison of the energy in bonds?
A. It is less than −600 kJ/mol, and the amount of energy required to break bonds is greater than the amount of energy released in forming bonds.

B. It is less than −600 kJ/mol, and the amount of energy required to break bonds is less than the amount of energy released in forming bonds.

C. It is greater than −600 kJ/mol, and the amount of energy required to break bonds is greater than the amount of energy released in forming bonds.

D. It is greater than −600 kJ/mol, and the amount of energy required to break bonds is less than the amount of energy released in forming bonds.

Answer 1

Answer:

C. It is greater than -600 kJ/mol, and the amount required to break bonds is greater than the amount of energy released in forming bonds.  

Explanation:

As a reaction occurs, bonds of reactants are broken and new bonds are formed in products. During bond breaking energy is absorbed while during bond formation energy is released. If the energy released during bond formation is greater than the energy absorbed during bond breaking, then the reaction is exothermic. If the energy released during bond formation is less than energy absorbed during bond breaking, then the reaction is endothermic.

If reactants have less energy than products, it means more energy is absorbed than released thus it is an endothermic reaction.

If reactants have more energy than products, it means more energy is released than absorbed thus it is an exothermic reaction.

Answer 2

Answer:

its c

Explanation:

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