Question

click the \investigation\ tab. the energy required to break a chemical bond is modeled by placing a molecule between the mechanical claws. place one of the hydrogen (h₂) molecules between the claws and click the \break bond\ button. remove the hydrogen atoms and repeat the procedure with the other h₂ molecule. remove the hydrogen atoms and place the oxygen (o₂) molecule between the claws. notice that the o₂ molecule is made up of a double bond. click the \break bond\ button twice to break apart the o₂ molecule. keep these settings for the next page. if you need help, there are instructions at the bottom of the \controls\ panel. enter the correct values in the boxes. total energy required to break both single h - h bonds: kj/mol total energy required to break both bonds in the o = o molecule: kj/mol total energy absorbed to break all the bonds: kj/mol

Explanation:

Step1: Recall bond - energy values

The bond - energy of a single H - H bond is approximately 436 kJ/mol. Since we have two H - H bonds, the total energy to break them is \(2\times436\) kJ/mol.
\[2\times436 = 872\]

Step2: Recall O=O bond - energy

The bond - energy of a double O=O bond is approximately 498 kJ/mol. Since we break one O=O double - bond (by clicking the "Break bond" button twice), the energy required is 498 kJ/mol.

Step3: Calculate total energy

The total energy absorbed to break all the bonds is the sum of the energy to break the H - H bonds and the O=O bond. So, \(872 + 498=1370\) kJ/mol.

Answer:

Total energy required to break both single H - H bonds: 872 kJ/mol
Total energy required to break both bonds in the O=O molecule: 498 kJ/mol
Total energy absorbed to break all the bonds: 1370 kJ/mol