alexignite/chemset1 · Datasets at Hugging Face

title stringlengths 8 78	text stringlengths 3 643
Cell voltage example .txt	It gains those electrons that are released by this zinc solid metal.
Cell voltage example .txt	So that means in step two, when we draw our electrochemical cell, the first half cell will contain our zinc solid.
Cell voltage example .txt	And that's because zinc is oxidized, and the anode always contains the oxidation reaction.
Cell voltage example .txt	So this is our zinc metal.
Cell voltage example .txt	That means this must be our cadmium metal.
Cell voltage example .txt	And so electrons will travel via the conductor, via this volt meter and into this cathode, into this electrode.
Cell voltage example .txt	The volt meter, by the way, is the thing that reads zero point 36 volts.
Cell voltage example .txt	So this sold bridge is placed here because it plays the role of closing the circuit.
Cell voltage example .txt	Without the sole bridge, this guy would not function.
Cell voltage example .txt	Electrons would not flow, and it's very important.
Cell voltage example .txt	So, once again, our anode, our place where oxidation occurs, and our cathode, the place where reduction occurs.
Cell voltage example .txt	So electrons travel from this way, from this electrode to this electrode.
Cell voltage example .txt	So when they leave this cell, this solid zinc releases electrons, right?
Cell voltage example .txt	Electrons begin to flow here.
Cell voltage example .txt	It also releases a zinc ion into this solution.
Cell voltage example .txt	And when the electrons travel this way, they combine.
Cell voltage example .txt	When they reach this metal, they combine with the cadmium ions forming our cadmium solid.
Cell voltage example .txt	So, in the third step, we basically want to use this cell voltage formula to find our cell voltage for the cathode.
Cell voltage example .txt	Remember?
Cell voltage example .txt	Now, we know that this guy, this value of negative zero point 76 represents the value for the anode.
Cell voltage example .txt	So we use this formula to solve for our cathode.
Cell voltage example .txt	So we know our 0.36 volts, which is told by the voltmeter.
Cell voltage example .txt	Now, this we don't know.
Cell voltage example .txt	So we let a DX minus now in parentheses we have a negative 0.76 volts, right?
Cell voltage example .txt	So negative and negative becomes a positive.
Cell voltage example .txt	Then we subtract both sides by this guy and we get x to be 0.36 -0.76 volts gives us negative 0.4 volts.
Cell voltage example .txt	So this is our cell voltage for the cathode cell for the cadmium for that reduction reaction of cadmium.
Charles Law .txt	Now we already spoke about a concept called the Kinetic Molecular Theory of Gases.
Charles Law .txt	And what this theory did for us is it helped us gain more intuition about how individual gas molecules interact on a very small microscopic level.
Charles Law .txt	Now we also spoke about a law called Boils Law.
Charles Law .txt	And what Boils Law did for us is it helps help us gain more intuition about the macroscopic behavior of gases.
Charles Law .txt	In other words, what happens at constant temperature when we take a balloon filled with air and squeeze it.
Charles Law .txt	Well, we said that, and Boyle's Law explained this, that when we squeeze the balloon, we decrease volume, increase pressure, and eventually our balloon will pop.
Charles Law .txt	Now we're going to look at another law called Charles Law which also helps us explain the macroscopic large scale behavior of many gas molecules and how they interact with one another and with our system.
Charles Law .txt	So for Charles Law to work, two conditions must hold.
Charles Law .txt	We must have constant pressure and we must have constant number of molecules.
Charles Law .txt	So our N number of moles stays the same.
Charles Law .txt	And what Charles Law does is it relates volume and temperature.
Charles Law .txt	Remember Boyle's Law related volume and pressure?
Charles Law .txt	Well, Charles Law relates temperature and volume when pressure is constant.
Charles Law .txt	And what it says is that volume is directly proportional to temperature.
Charles Law .txt	And this means if we bring the T over or if we multiply a constant by T and we bring T over, what we get is the following v divided by T is equal to a constant.
Charles Law .txt	Remember, in Boyle's Law we saw that P times V gave us a constant and that if we increase pressure, our volume must decrease while keeping the constant the same.
Charles Law .txt	Well, in this case, we have the same kind of situation, except now we have volume divided by temperature.
Charles Law .txt	In other words.
Charles Law .txt	Now for this constant to remain a constant and not change if we increase volume, say by two, our temperature also must increase by the same amount by two.
Charles Law .txt	So whenever we increase volume, we increase temperature.
Charles Law .txt	Or if we decrease volume, we must decrease the temperature for this guy to remain constant.
Charles Law .txt	Now notice this constant remains or depends on two things on the pressure and on the number of molecules.
Charles Law .txt	For example, if we have more molecules, our constant will be higher.
Charles Law .txt	And we'll learn more about that when we talk about the ideal gas law.
Charles Law .txt	For now, it's sufficient to say that our cost depends on both of these guys.
Charles Law .txt	So the same way we did for Boyle's Law, for Charles Law, we can rewrite this relation or this relation in the following manner.
Charles Law .txt	Now, suppose I have some system, some gas system and I have two sets of different conditions for this gas system.
Charles Law .txt	Well, I can relate them in the following manner.
Charles Law .txt	Assuming that these guys are both constant.
Charles Law .txt	In other words, note that the constant always stays the same when our pressure number of moles stays the same.
Charles Law .txt	That means if we have some conditions, v one and T one and a second condition of V two and T two.
Charles Law .txt	And these two conditions are under the same pressure and number of moles, that means our constant will be the same.
Charles Law .txt	And so I can say V one over T one equals V two over t two equals that same constant.
Charles Law .txt	So once again, for a gas sample with two different sets of T's and Vs for two different conditions, this is our law.
Charles Law .txt	This is our Charles Law.
Charles Law .txt	Now, whenever we talk about gases, and we talk about these different laws that revolve around gases, our temperature is never in Celsius, it's only in Kelvin.
Charles Law .txt	And that means we have to convert Celsius to Kelvin.
Charles Law .txt	And this is how you do it.
Charles Law .txt	To get the Kelvin temperature, you take the Celsius temperature and you add 273.15 to it.
Charles Law .txt	For example, if our Celsius temperature is ten degrees Celsius, I simply add 273.15 and I get 283.15 Kelvin.
Charles Law .txt	That's our temperature in Kelvin.
Charles Law .txt	So let's think of an example where Charles Law is evident.
Charles Law .txt	So suppose it's someone's birthday and it's winter.
Charles Law .txt	So it's cold outside and you need to go and buy somebody a present.
Charles Law .txt	So he decides to buy a balloon.
Charles Law .txt	So you go inside the store, you fill up the balloon with some helium.
Charles Law .txt	Now suppose once you fill the balloon up, there are no holes in the balloon.
Charles Law .txt	So the number of moles or number of molecules inside our balloon remains constant.
Charles Law .txt	Also, let's suppose that our pressure inside the store and outside is one ATM atmospheric pressure.
Charles Law .txt	So let's suppose that our pressure is also constant.
Charles Law .txt	Now, obviously, if it's winter, it's much colder outside than inside.
Charles Law .txt	So suppose I fill up my balloon with N number of moles of helium, and suppose now I go outside with that balloon.
Charles Law .txt	Well, on the inside, inside the store, we were at one condition.
Charles Law .txt	We had some D two and t two, right?
Charles Law .txt	Once we step outside, our temperature drops.
Charles Law .txt	So what happens to volume?
Charles Law .txt	Well, according to Charles Law, this guy states that if we go outside and my temperature drops, then my volume must drop as well to make sure that our constant stays the same.
Charles Law .txt	That means if I go outside with my balloon, my balloon will shrivel, it will become smaller, and that's because of Charles Law.
Charles Law .txt	So once again, we see how macro scale events are explained by Charles Law, just like they were explained by Boyle's Law.
Charles Law .txt	So we have yet another law that helps us explain how gas molecules behave when we have a lot of them together, not simply individual gas molecules.
Charles Law .txt	Now, we can, of course, explain how Charles Law functions on an individual level using the kinetic theory.
Charles Law .txt	Now, kinetic theory explains Charles Law on a microscopic level at constant pressure.
Charles Law .txt	So we have constant pressure, right?
Charles Law .txt	Our pressure doesn't change.
Charles Law .txt	So if our temperature increases, what happens to the molecules?
Charles Law .txt	The molecules gain more kinetic energy.
Charles Law .txt	And if they gain more kinetic energy, they gain more speed.
Charles Law .txt	They become quicker.
Charles Law .txt	And that means the only way that our pressure stays constant with higher kinetic energy is if the volume expands.
Charles Law .txt	So that's exactly what happens.
Charles Law .txt	In order to ensure that there is constant pressure.
Charles Law .txt	An increase in temperature means there's an increase in kinetic energy.
Charles Law .txt	And this increase in kinetic energy means that there are more molecules, or the molecules are pushing against the wall of the container with greater force.

Cell voltage example .txt

It gains those electrons that are released by this zinc solid metal.

Cell voltage example .txt

So that means in step two, when we draw our electrochemical cell, the first half cell will contain our zinc solid.

Cell voltage example .txt

And that's because zinc is oxidized, and the anode always contains the oxidation reaction.

Cell voltage example .txt

So this is our zinc metal.

Cell voltage example .txt

That means this must be our cadmium metal.

Cell voltage example .txt

And so electrons will travel via the conductor, via this volt meter and into this cathode, into this electrode.

Cell voltage example .txt

The volt meter, by the way, is the thing that reads zero point 36 volts.

Cell voltage example .txt

So this sold bridge is placed here because it plays the role of closing the circuit.

Cell voltage example .txt

Without the sole bridge, this guy would not function.

Cell voltage example .txt

Electrons would not flow, and it's very important.

Cell voltage example .txt

So, once again, our anode, our place where oxidation occurs, and our cathode, the place where reduction occurs.

Cell voltage example .txt

So electrons travel from this way, from this electrode to this electrode.

Cell voltage example .txt

So when they leave this cell, this solid zinc releases electrons, right?

Cell voltage example .txt

Electrons begin to flow here.

Cell voltage example .txt

It also releases a zinc ion into this solution.

Cell voltage example .txt

And when the electrons travel this way, they combine.

Cell voltage example .txt

When they reach this metal, they combine with the cadmium ions forming our cadmium solid.

Cell voltage example .txt

So, in the third step, we basically want to use this cell voltage formula to find our cell voltage for the cathode.

Cell voltage example .txt

Remember?

Cell voltage example .txt

Now, we know that this guy, this value of negative zero point 76 represents the value for the anode.

Cell voltage example .txt

So we use this formula to solve for our cathode.

Cell voltage example .txt

So we know our 0.36 volts, which is told by the voltmeter.

Cell voltage example .txt

Now, this we don't know.

Cell voltage example .txt

So we let a DX minus now in parentheses we have a negative 0.76 volts, right?

Cell voltage example .txt

So negative and negative becomes a positive.

Cell voltage example .txt

Then we subtract both sides by this guy and we get x to be 0.36 -0.76 volts gives us negative 0.4 volts.

Cell voltage example .txt

So this is our cell voltage for the cathode cell for the cadmium for that reduction reaction of cadmium.

Charles Law .txt

Now we already spoke about a concept called the Kinetic Molecular Theory of Gases.

Charles Law .txt

And what this theory did for us is it helped us gain more intuition about how individual gas molecules interact on a very small microscopic level.

Charles Law .txt

Now we also spoke about a law called Boils Law.

Charles Law .txt

And what Boils Law did for us is it helps help us gain more intuition about the macroscopic behavior of gases.

Charles Law .txt

In other words, what happens at constant temperature when we take a balloon filled with air and squeeze it.

Charles Law .txt

Well, we said that, and Boyle's Law explained this, that when we squeeze the balloon, we decrease volume, increase pressure, and eventually our balloon will pop.

Charles Law .txt

Now we're going to look at another law called Charles Law which also helps us explain the macroscopic large scale behavior of many gas molecules and how they interact with one another and with our system.

Charles Law .txt

So for Charles Law to work, two conditions must hold.

Charles Law .txt

We must have constant pressure and we must have constant number of molecules.

Charles Law .txt

So our N number of moles stays the same.

Charles Law .txt

And what Charles Law does is it relates volume and temperature.

Charles Law .txt

Remember Boyle's Law related volume and pressure?

Charles Law .txt

Well, Charles Law relates temperature and volume when pressure is constant.

Charles Law .txt

And what it says is that volume is directly proportional to temperature.

Charles Law .txt

And this means if we bring the T over or if we multiply a constant by T and we bring T over, what we get is the following v divided by T is equal to a constant.

Charles Law .txt

Remember, in Boyle's Law we saw that P times V gave us a constant and that if we increase pressure, our volume must decrease while keeping the constant the same.

Charles Law .txt

Well, in this case, we have the same kind of situation, except now we have volume divided by temperature.

Charles Law .txt

In other words.

Charles Law .txt

Now for this constant to remain a constant and not change if we increase volume, say by two, our temperature also must increase by the same amount by two.

Charles Law .txt

So whenever we increase volume, we increase temperature.

Charles Law .txt

Or if we decrease volume, we must decrease the temperature for this guy to remain constant.

Charles Law .txt

Now notice this constant remains or depends on two things on the pressure and on the number of molecules.

Charles Law .txt

For example, if we have more molecules, our constant will be higher.

Charles Law .txt

And we'll learn more about that when we talk about the ideal gas law.

Charles Law .txt

For now, it's sufficient to say that our cost depends on both of these guys.

Charles Law .txt

So the same way we did for Boyle's Law, for Charles Law, we can rewrite this relation or this relation in the following manner.

Charles Law .txt

Now, suppose I have some system, some gas system and I have two sets of different conditions for this gas system.

Charles Law .txt

Well, I can relate them in the following manner.

Charles Law .txt

Assuming that these guys are both constant.

Charles Law .txt

In other words, note that the constant always stays the same when our pressure number of moles stays the same.

Charles Law .txt

That means if we have some conditions, v one and T one and a second condition of V two and T two.

Charles Law .txt

And these two conditions are under the same pressure and number of moles, that means our constant will be the same.

Charles Law .txt

And so I can say V one over T one equals V two over t two equals that same constant.

Charles Law .txt

So once again, for a gas sample with two different sets of T's and Vs for two different conditions, this is our law.

Charles Law .txt

This is our Charles Law.

Charles Law .txt

Now, whenever we talk about gases, and we talk about these different laws that revolve around gases, our temperature is never in Celsius, it's only in Kelvin.

Charles Law .txt

And that means we have to convert Celsius to Kelvin.

Charles Law .txt

And this is how you do it.

Charles Law .txt

To get the Kelvin temperature, you take the Celsius temperature and you add 273.15 to it.

Charles Law .txt

For example, if our Celsius temperature is ten degrees Celsius, I simply add 273.15 and I get 283.15 Kelvin.

Charles Law .txt

That's our temperature in Kelvin.

Charles Law .txt

So let's think of an example where Charles Law is evident.

Charles Law .txt

So suppose it's someone's birthday and it's winter.

Charles Law .txt

So it's cold outside and you need to go and buy somebody a present.

Charles Law .txt

So he decides to buy a balloon.

Charles Law .txt

So you go inside the store, you fill up the balloon with some helium.

Charles Law .txt

Now suppose once you fill the balloon up, there are no holes in the balloon.

Charles Law .txt

So the number of moles or number of molecules inside our balloon remains constant.

Charles Law .txt

Also, let's suppose that our pressure inside the store and outside is one ATM atmospheric pressure.

Charles Law .txt

So let's suppose that our pressure is also constant.

Charles Law .txt

Now, obviously, if it's winter, it's much colder outside than inside.

Charles Law .txt

So suppose I fill up my balloon with N number of moles of helium, and suppose now I go outside with that balloon.

Charles Law .txt

Well, on the inside, inside the store, we were at one condition.

Charles Law .txt

We had some D two and t two, right?

Charles Law .txt

Once we step outside, our temperature drops.

Charles Law .txt

So what happens to volume?

Charles Law .txt

Well, according to Charles Law, this guy states that if we go outside and my temperature drops, then my volume must drop as well to make sure that our constant stays the same.

Charles Law .txt

That means if I go outside with my balloon, my balloon will shrivel, it will become smaller, and that's because of Charles Law.

Charles Law .txt

So once again, we see how macro scale events are explained by Charles Law, just like they were explained by Boyle's Law.

Charles Law .txt

So we have yet another law that helps us explain how gas molecules behave when we have a lot of them together, not simply individual gas molecules.

Charles Law .txt

Now, we can, of course, explain how Charles Law functions on an individual level using the kinetic theory.

Charles Law .txt

Now, kinetic theory explains Charles Law on a microscopic level at constant pressure.

Charles Law .txt

So we have constant pressure, right?

Charles Law .txt

Our pressure doesn't change.

Charles Law .txt

So if our temperature increases, what happens to the molecules?

Charles Law .txt

The molecules gain more kinetic energy.

Charles Law .txt

And if they gain more kinetic energy, they gain more speed.

Charles Law .txt

They become quicker.

Charles Law .txt

And that means the only way that our pressure stays constant with higher kinetic energy is if the volume expands.

Charles Law .txt

So that's exactly what happens.

Charles Law .txt

In order to ensure that there is constant pressure.

Charles Law .txt

An increase in temperature means there's an increase in kinetic energy.

Charles Law .txt

And this increase in kinetic energy means that there are more molecules, or the molecules are pushing against the wall of the container with greater force.