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Gay-Lussac's law: The P-T relationship at constant volume
Gas Laws: Gay-Lussac's Law
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On the previous page we saw the relationship between temperature and volume (at constant pressure and number of particles). Let's now alter those parameters slightly but swapping constant pressure for constant volume. That is, we'll again raise the temperature of the gas, but this time the size of the container will be fixed. The piston will be locked in place.
Let's run the simulator and see if you were correct.
Instructions:
1. Click the Increase Temperature button to slowly increase the temperature (note that unlike our last simulation, the piston is now in a fixed position). Observe how the pressure changes as we increase the temperature. Let the simulator run until it stops automatically.
3. Take a snapshot of the graph as you did before. When the Add Snapshot dialog box appears, type "Pressure vs. Temperature at constant volume and number of particles" in the box below the snapshot. Click OK.
Was your prediction from the top of the page correct? Did the pressure change as you expected?
As we increased the temperature, we discovered that the pressure increased because the rate and strength with which the gas molecules collided with the container walls increased.
This direct relationship between temperature and pressure is known as Gay-Lussac's law. Later in this activity, we'll see how Gay-Lussac's law explains how autoclaves work.
Now that we've seen Boyle's law (inverse relationship between pressure and volume), Charles's law (direct relationship between temperature and volume), and Gay-Lussac's law (direct relationship between temperature and pressure) let's move on to our fourth and final gas law where we'll explore the relationship between volume and the number of particles of a gas.
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pressure will decrease because the rate and strength of the collisions with the container wall will decrease
pressure will decrease because the rate and strength of the collisions with the container wall will increase
pressure will increase because the rate and strength of the collisions with the container wall will decrease
pressure will increase because the rate and strength of the collisions with the container wall will increase
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<font size="3" face="verdana">As the temperature increased, what happened
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pressure increased
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<font size="3" face="verdana">Predict what would have happened to the
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pressure would have decreased
pressure would have increased
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