And looking at our equation, if the number of microstates increases, then so does the entropy. Of possible positions for the gas particles. When the volume is doubled, that increases the number Next, let's think about what happens to the number of available microstates when the volume is doubled. Therefore, the initial temperature, T1, is equal to the final temperature, T2. During the expansion of the gas, the temperature is kept constant. Mole of our ideal gas and n2 is also equal to one mole. Volume for the final volume, therefore, V2, or the final volume, is equal to 2 times V1. So if the initial volume is V1, let's say we have twice the
#Entropy definition chemistry free
And now our gas particlesĪre free to travel around in a larger volume. Let's say we go aheadĪnd remove the divider.
Particles, in a container, and the container has a removable divider separating the container One mole of an ideal gas, so here are the gas In our first situation, we're starting off with The change in entropy for a number of different situations. Of either matter or energy, that really relates to a decrease in the number of available microstates, which means a decrease in And if we think about aĭecrease in the disorder of the system or an increase in the order, or a decrease in the dispersal Terms as meaning an increase in the number of microstates and therefore an increase in However, when we're using the equationĭeveloped by Boltzmann, we should think about these Using the word microstates, people will describeĪn increase in entropy as an increase in disorder or an increase in the dispersal Microstates decreases, that represents a decrease Of a system increases, that represents an increase in entropy, and if the number of According to this equation, entropy, symbolized by S, is equal to Boltzmann's constant, k, times the natural log of W, and W represents the number Now that we understand theĬoncept of microstates, let's look at an equationĭeveloped by Boltzmann that relates entropy to Is a number that's too high for us to even comprehend. So the number of microstatesĪvailable to this system of one mole of gas particles Moving from one microstate into another, into another, into another. The microscopic level, we see that the system is So from a macroscopic point of view, nothing seems to change. A good way to think aboutĪ microstate would be like taking a picture of
Microscopic arrangement of positions and energies So going back to our boxes,īox 1, box 2 and box 3, each box shows a different To the kinetic energies of the particles. With an ideal gas here, by energies, we're referring Microscopic arrangement of all of the positions andĮnergies of the gas particles. Of each particle is equal to 1/2 mv squared, where m is the mass of each Particles are meant to represent the velocities of the particles. And the magnitude and theĭirection give a velocity. However, when we put anĪrrow on each particle, that also gives us the direction. Of a particle tells us how fast the particle is traveling. Slightly different positions and the velocities might have changed. Particles in our system at one moment in time, in box 1, if we think about them atĪ different moment in time, in box 2, the particles might be in Slamming into each other and transferring energy from Slamming into the sides of the container and maybe Here in the first box, imagine these gas particles However, from a microscopic point of view, things are changing all of the time. So from a macroscopic point of view, nothing seems to be changing. Particles is at equilibrium, then the pressure, the volume, the number of moles, and the temperature all remain the same. Moles at a specific pressure, volume, and temperature. And to think about microstates, let's consider one mole of an ideal gas.
Of entropy is related to the idea of microstates.
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