2C2H2 + 5O2 -> 4CO2 + 2H2O + energy

What does the equation communicate about the relative energy of the chemical bonds in the reactants and products?

The intermolecular bonds of the reactants are weaker than that of the products' because the products' intermolecular bonds broke easily, meaning less energy was required to break the bonds of the reactants than was made when the products' bonds were formed. Thus, more energy was released.

First of all, is that right? And I think the wording can use some work, if someone could help me with making a better explanation, I'd be extremely grateful.

That sound ok to me. It may not win a Pulitzer Prize but I think it covers the subject ok.

If you absolutely had to improve it what would you improve? Anything that sticks out especially to you

But thank you; haha, I wouldn't go after an American prize anyways!

The intermolecular bonds of the reactants are weaker than that of the products' because the products' intermolecular bonds broke easily, meaning less energy was required to break the bonds of the reactants than was made when the products' bonds were formed. Thus, more energy was released.

The bonds of the reactants are weaker than those of the products. Less energy was required to break the bonds of the reactants than was formed for the products and energy was released in an exothermic reaction..

Well, the chemical equation you provided is a combustion reaction of acetylene (C2H2). So, let's see if we can come up with a clownish way to explain it!

Ah, the magical dance of molecules! In this fiery tango, the reactants C2H2 and O2 join forces to form the products CO2 and H2O. But what about energy? Ah, yes, the party crasher!

You see, my dear friend, the reactants' intermolecular bonds are not quite as strong as those in the products. The reactants' bonds are like those flimsy balloons that pop easily, requiring less energy to break. But oh, when those products' bonds form, it's like a fortress building itself! It takes more energy to break them apart.

So, as the reaction dances on, energy is released into the wild, spreading joy and warmth to the world. The reactants' bonds were like little energy prisoners, and the products' bonds, oh boy, they were like energy superheroes, freeing the energy and throwing a wild party!

I hope this whimsical explanation makes you smile, my friend!

Your explanation is almost correct, but let's refine it a bit for better clarity.

The given chemical equation for the reaction shows the conversion of 2 molecules of C2H2 (acetylene) and 5 molecules of O2 (oxygen) into 4 molecules of CO2 (carbon dioxide) and 2 molecules of H2O (water), along with the release of energy.

The energy released in the reaction indicates that the products have stronger intermolecular bonds compared to the reactants. This is because breaking the intermolecular bonds of the reactants required less energy than was released when the products' bonds were formed.

To explain it more precisely, the breaking of the C-C and H-H bonds in acetylene (C2H2) and the O=O bonds in oxygen (O2) required a relatively small amount of energy input. However, the formation of the new C=O bonds in carbon dioxide (CO2) and the O-H bonds in water (H2O) released a larger amount of energy.

As a result, the net energy change is negative, indicating an exothermic reaction where energy is released. This suggests that the products are more stable and have stronger intermolecular bonds than the reactants.