explain-why-the-liquid-in-the-barometer-does-not-spill-out-2

Name: explain why the liquid in the barometer does not spill out 2
Uploaded: 2020-10-14
Duration: 1 min 2 s
Channel: Numerade
Description: Explain why the liquid in the barometer does not spill out.

Question

Explain why the liquid in the barometer does not spill out.

David Collins · Accepted Answer

the liquid in a barometer does not spill out. Really, for two reasons. One is in the barometer, there&#x27;s a vacuum at the top, and the vacuum is pulling well. It&#x27;s pulling because theater mus fear is pushing, so that&#x27;s probably a better way to put it. And then the mercury is rising, and we have atmospheric pressure pushing down on the mercury because there&#x27;s a vacuum up here than the height of the Mercury column equals the pressure of the atmosphere. So it&#x27;s not spilling out because theater a sphere is pushing it in and keeps pushing it in according to the pressure of the atmosphere.

Charotte Mcadam · Answer

So we&#x27;re continuing our winter topic of pressure here, and so just drop some context. We have some definitions to consider. So if the first one is a fire a meter. So this is an instrument that is used to measure atmospheric pressures. So it is made up of uninvited tube in a dish that is filled up with mercury next week, and it can look at a man a meter. So this is a device that is used to measure the pressure off fluid so it has a U shaped tube on it is filled with it, just some non volatile liquid. So we have two types off mana meters. We have the open end on the closed end versions. So for gas is pressures lesser than atmospheric pressure. The closed down manna meter is used, whereas the open ended man ometer is used for all cases. So if we have a volatile liquid that is one that can evaporate at low temperature, then if a volatile liquid is used in a man ometer or borrow meter, then the measured pressure will be due to gas as well as due to vapors off the volatile liquid. So therefore, the exact pressure cannot be determined, so the non volatile liquid evaporates very high temperatures on DSO. It does not evaporate at room temperature. Therefore, the measured pressure will be only due to gas. So therefore, when we have a non volatile liquid, this is always used in a bar. Amita, an Amman, Amita.

Abdel Osman · Answer

and this question were given that to evacuated balls of equal volume are connected by a two of negligible volume. One mole of an ideal guys is injected into the system and one of the bulbs is in a different temperature and the other and were asked to calculate the final number of moles of gas in each boat. So, first, we&#x27;re gonna start off with the ideal gas law. PV equals NRT. Now we know that the volume of each bulb are equal. And given this, we can also say that the pressure in each bulb is also equal because these are directly I&#x27;m sorry, there inversely proportional to each other. Now, based on this, we can actually set up a different equation and that is an arty equal to NRT of the other book. We can cross out the ours we&#x27;re left with n a t A equals nb TB. Now we&#x27;re trying to find the number of bowls of in each bulb. So let&#x27;s go ahead and first, all for an eight. So we&#x27;re gonna move ta to the other side and we&#x27;re actually given that to the temperature and one bulb is 350 Kelvin. The other one is 225 Calvin. So based on this, we can actually create a ratio to 25. Divided by 3 50 is going to be around 0.64 three. Now, from here we can do some math. But first we have to realize something we inject from one mole of this ideal gas. So no matter what happens, an A plus and be has to equal one more. But now, if you take a look, we&#x27;ve already set any equal to something So we can do and be multiplied by 0.643 plus NB equals one. So now we have 1.643 equals one. Can we find that the most we have in one of the bulbs is 1/1 0.643? We&#x27;re just equal to 0.61 moles. So here are the amount of moles in one bulb

Shivani Naidu · Answer

mercury is used in a barometer rather than water because mercury has a higher density than water, which means the height of the column needed for mercury will be lower than that off water. Mercury also has a low way per pressure, so it will not evaporate easily. Mercury stays liquid at a wide variety of temperatures, so it&#x27;s easy to measure pressure at various temperatures. Mercury also does not stick to glass.

Marissa Turner · Answer

This is a problem. Five from Chapter 11 gases. And it&#x27;s asking why mercury is better than water for measuring pressure. So mercury has been used due to the higher density so and it helps construct the barometer and nanometer. So you all know that water has a density of one gram for a meal later. Mercury has about 13.5 grants from no leader propensity, so tired by that so basically of mercury Sands one meter tall or barometer, so mercury on his down one year tall, where&#x27;s water has to be at least 13 meters tall?

Anatole Borisov · Answer

So what&#x27;s happening here is we&#x27;re discussing the way Ah, liquid vaporizes into a gas. And so here we have some red liquid right here and throughout. At the surface, we have molecules that will evaporate and become gas, thus training a vapor pressure. And we also have molecules in the solution that aren&#x27;t near the surface. And they have a lot of energy they might be, you know, there&#x27;s whizzing around in there, and they might have enough energy to becoming gaps, and they might momentarily approach that state, and they might become a gas. But the issue is that the rest of the molecules around them there&#x27;s such a high pressure of water on. And there&#x27;s so many water molecules have saying water. There&#x27;s so many liquid ball feels around there that theatre collective force between them and this newly formed gas. We&#x27;re just going to snuff out that little little potential of like vapor, and so it&#x27;s going to go back to just being a little other liquid. However, if we turn up the heat, what that does is that gives these molecules mawr energy to break the overcome the Inter Michler forces between them so say this molecule right here, it&#x27;s whizzing around. It&#x27;s fast, it&#x27;s got the energy, you becomes a gas, and now it&#x27;s numb. The molecules around it don&#x27;t have enough strength compared to the height, higher temperature, the higher energy that this molecule has to really bag in to use its instrument but forces to make it look again in this gas escapes. And that&#x27;s what&#x27;s happening when it&#x27;s boiling. And so, in summary, the answer is that the reason paper doesn&#x27;t form throughout a liquid lower than its boiling point is because the enemy, like our forces of the neighboring molecules, are not over time. They&#x27;re much stronger than if the that one tiny gas part molecule that could exist in there and it gets snuffed out.

Problem 8 Easy Difficulty

Explain why the liquid in the barometer does not spill out.

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