# Pressure and number of moles relationship quiz

### Ideal Gas Law Formula The relationships between the following four variables are known as the gas laws . stapelholm.info (H, in cm), volume (V), temperature (T), and amount (n, in moles) (V ) of a fixed amount of gas is inversely proportional to its pressure (P) is called. It predicts specific relationships between pressure, temperature, volume and the number of moles of gas present, relationships that are summarized in the Ideal Gas Law To complete this lesson, you should try the self quiz in your workbook. Do pressure and temperature have a direct or inverse relationship? Direct . The number of moles of gas, its volume and temperature. Science Quiz #3.

I then pass out the quiz to students. I have two versions of the quiz to ensure academic honesty and give them so that students have a different version from the person next to or across from them.

This is a copy of the quiz.

### Ninth grade Lesson The Ideal Gas Law and Dalton's Law of Partial Pressures

As students complete their quizzes I have them turn over and then come around to collect. I give students about 10 minutes to complete the quiz. When students are done if I have collected their quiz then I encourage them to get out their binders and begin to get ready for the lesson. After class I grade the quizzes using the answer key and place in my gradebook. See the attached reflection for more details about how I do quiz corrections. I begin the lesson with teaching students about the Ideal gas law on slide 2. I also tell students that there are multiple "R" values, but that for this class we will only be using 0. I then have students do the practice questions on slides I make sure that students use the problem solving technique of underlining what they know, circling what they want, labeling, writing down the equation, isolating their variable, and then solving for the answer.

## Properties of Gases

In the first example students have to first convert mL to L. I have them do this to review this type of conversion. In the second example students need to first convert grams to moles using molar mass.

I give them the hint that they will need their periodic tables for this. I can add heat. If I added ten joules of heat I'd add ten joules to the internal energy, but I've also got to take into account this work being done, and so I can do plus the work done on the gas, and that's it, this is actually the first law of thermodynamics, it's the law of conservation of energy it says there's only two ways to add energy, internal energy to a gas.

Let me talk a little bit more about this work done though cause getting the sign right is important. If you're doing work on the gas compressing it you're adding energy to the gas, but if you let the gas push up on the piston and this gas expands pushing the piston up, then the gas is doing the work, that's energy leaving the system. So if the gas does work you have to subtract work done by the gas. If the outside force does work on the gas you add that to the internal energy.

So you got to pay attention to which way the energy is flowing. Work done on gas, energy goes in. Work done by the gas, energy goes out, and you'd have to subtract that over here. Let's say the gas did expand. Let's say the gas in here was under so much pressure that the force it exerted on this piston was enough to push that piston upward by a certain amount. So let's say it started right here and it went up to here so that piston went from here to there no gasses escaping cause this is tightly fitting, but the gas was able to push it up a certain distance d, how much work was done?

You know the definition of work. Work is defined to be the force times the distance through which that force was applied. So the work that the gas did was F times d, but we want this to be in terms of thermal quantities like pressure, and volume, and temperature. So what could we do? We can say that this volume, not only did the piston raise up, but there was an extra volume generated within here that I'm going to call Delta V, and I know that this Delta V has got to equal the area of the piston times the distance through which that piston moved because this height times that area gives me this volume right in here.

Why am I doing this? Cause look I can write d as equal to Delta V over A, and I can take this, I can substitute this formula for d into here, and something magical happens, I'll get work equals F times Delta V over A, but look F over A, we know what F over A is, that's pressure so I get that the work done by the gas is the pressure times Delta V.

This is an equation that I like because it's in terms of thermodynamic quantities that we're already dealing with. So work done you can figure out by taking P times Delta V but strictly speaking this is only true if this pressure remained constant, right? If the pressure was changing, then what am I supposed to plug in here, the initial pressure, the final pressure?

If the pressure's staying constant this gives you an exact way to find the work done.

• Lesson 1: Wrap Up
• The Ideal Gas Law and Dalton's Law of Partial Pressures
• Ideal Gas Law Formula

You might object and say wait, how is it possible for a gas to expand and remain at the same pressure? Well, you basically have to heat it up while the gas expands, that allows the pressure to remain constant as the gas expands.

And now we're finally ready to talk about heat capacities. So let's get rid of this, and heat capacity is defined to be, imagine you had a certain amount of heat being added. So a certain amount of heat gets added to your gas.

How much does the temperature increase? That's what the heat capacity tells you.

### PV=nRT Relationship quiz - By Jabroach09

So capital C is heat capacity and it's defined to be the amount of heat that you've added to the gas, divided by the amount of change in the temperature of that gas. And actually, something you'll hear about often is the molar heat capacity, which is actually divided by an extra n here.

Pretty simple but think about it. If we had a piston in here, are we going to allow that piston to move while we add the heat, or are we not going to allow the piston to move? There's different ways that this can happen, and because of that there's different heat capacities. If we don't allow this piston to move, if we weld this thing shut so it can't move we've got heat capacity at constant volume, and if we do allow this piston to move freely while we add the heat so that the pressure inside of here remains constant, we'd have the heat capacity at constant pressure.

And these are similar but different, and they're related, and we can figure them out. So let's clear this away, let's get a nice, here we go, two pistons inside of cylinders. We'll put a piston in here, but I'm going to weld this one shut. This one can't move. We'll have another one over here, it can move freely. So over on this side, we'll have the definition of heat capacity, regular heat capacity, is the amount of heat you add divided by the change in temperature that you get.