Explain Avogadro's law using the kinetic–molecular theory of gase...

Question

Explain Avogadro's law using the kinetic–molecular theory of gases.

Accepted Answer

Welcome back, everyone. Which of the following based on kinetic molecular theory of gasses best explains Avogadro's law. We have choice A which states that Avogadro's law is going to be valid independent of chemical identity of the gas. And that's because the volume of space occupied by the gas molecules will be significantly less than the volume of space between molecules. Choice B states that Avogadro's law is valid dependent on chemical identity of the gas. Since the gas molecules are always moving quickly and randomly. And then choice C states that Avogadro's law is going to be valid independent of chemical identity of the gas since gas molecules won't have attractive or repulsive forces with each other. And then choice D states that Avogadro's law is valid dependent on the chemical identity of the gas. Since the temperature of the gas affects the average kinetic energy of the gas molecules. Let's begin by recalling that according to Avogadro's law, we have equivalent volumes of gasses at constant temperature And pressure. And because of these equivalent volumes, we can say that we have an equal number of molecules where N would equal N two. So next, let's recall that our kinetic molecular theory postulate describes small gas particles which are far apart from one another in comparison to their size. So we can note down that we have gas particles at a far distance versus their size. And we want to recall that according to kinetic molecular theory, the motion of gasses or the motion of gas particles and the distance between them Is going to be the number one factor which influences volume. And based on what we've outlined, we can therefore say that Avogadro's law is actually valid and this is independent of our gas identity. And this is based off of the fact from our kinetic molecular theory postulate that the volume of space between our molecules of gas is significantly greater than the volume of space occupied by the molecules of gas. And based on what we've outlined, because we know that Avogadro's law is valid independent of our gas identity, we would be able to rule out choices B as well as D, which state that Avogadro's law is valid dependent on the chemical identity. And then between choices A and C, we would rule out choice C because it mentions our lack of attractive and repulsive forces with the gas molecules to one another. And fails to mention the key point of our kinetic molecular theory postulate, which is the distance between our gas particles when in motion. And so, based on what we've outlined, we can confirm that the only correct choice would be choice. A which states that Avogadro's law is valid, independent of the chemical identity of the gas. Since the volume of space occupied by gas molecules is significantly less than the volume of space between molecules. So A is our final answer. I hope this made sense and let us know if you have any questions.

Explain Avogadro's law using the kinetic–molecular theory of gases.

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