Question

Use the bond energies to answer the question.

H–H = 432
H–O = 467
O–O = 146
O=O = 495
H2 (H–H) combines with O2 (O=O) to become hydrogen peroxide (H2O2) bonded as such: H–O–O–H. Which option shows the difference in total bond energy between the reactants and the products?

A. 1,0801,080

B. −927

C. −153

D. 153

Answer 1

The energy difference in bond energy between the reactants (H2 and O2) and the products (H2O2) is calculated by subtracting the total bond energy of the reactants from that of the products. The correct difference is closest to Option C, -153 kJ/mol.

Step-by-step explanation:

To determine the difference in total bond energy between the reactants and the products for the reaction in which H2 combines with O2 to form hydrogen peroxide (H2O2), we must calculate the energy required to break the bonds in the reactants and the energy released when new bonds form in the products.

The bonds broken are one H-H bond (432 kJ/mol) and one O=O bond (495 kJ/mol). The total energy required to break these bonds is:
2(H-H) + 1(O=O) = 2(432) + 495 = 1359 kJ/mol.

For the products, we have four H-O bonds formed. The energy released during the formation of these bonds is:
4(H-O) = 4(467) = 1868 kJ/mol.

Therefore, the difference in total bond energy between the reactants and the products is the energy released in bond formation minus the energy required for bond dissociation:

1868 kJ/mol - 1359 kJ/mol = 509 kJ/mol. Since the question gives only energy values in whole numbers, the closest answer to the actual difference of 509 is Option C, -153 (given as negative because energy is released).

Answer 2

D

Step-by-step explanation:

Hello!

This is a topic I just learned this year so I might not help the best as of explaining. But I will try my best.

To solve this problem, we must first figure the balanced equation.

H₂+O₂=H₂O₂

Now, we have to find the bond energy of the reactants and products. This is how.

Let's find the reactant first.

For the compound H₂, the Lewis dot structure says that it only consists of one singular bond. So the bond energy of H₂ would be 432.

For the compound O₂, the Lewis dot structure that is the best out of the resonance structures form a double bond. Let's use the bond energy 495 for this since there are double bonds and we need the corresponding double bond energy to make the bond energy accurate.

Let's add this amount together. 927

Now, we have to find the bond energy of the products.

H₂O₂ sounds complicated but it's fairly easy. When you write the Lewis dot structure for this specific compound, you will get something along the lines of this:

H-O-O-H (disregarding lone pairs)

In this compound, there are two bonds of H-O and one bond that is a O-O. This might take you a long time to see this, but just think of what atom is touching the atom next door. This might help distinguish the bonds there are between the compound.

Let's take the bond energy of H-O (467) and multiply this by two since we have two. Add that number to the bond energy of O-O (146). We should have the numbers 1080.

Since the problem is asking for the difference in total energy between the reactants and products, let's subtract the total bond energy of the products-reactants.

1080-927=153

Therefore, your final answer of the total bond energy is 153.