Term
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Definition
| The amount of force gas particles exert on the walls of their container, per unit area of the container |
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Term
| What is are the units of pressure (include conversions)? |
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Definition
| 760 torr = 750 mmHg = 1 atm |
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Term
| What are the two assumptions of the Ideal Gas Law? |
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Definition
1. Molecules of ideal gases do not attract or repel each other.
2. Molecules of ideal gases occupy zero volume. |
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Term
| In order to behave as an ideal gas, what two conditions must be satisfied? |
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Definition
1. Low pressure
2. High temperature |
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Term
| Explain kinetic molecular theory. In other words, what is the relationship between temperature and pressure in the Ideal Gas equation? |
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Definition
Directly proportional:
As temperature increases, molecules obtain more kinetic energy, which means they move around more. When molecules have more movement, they exert more pressure on container walls. |
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Term
| What is the relationship to volume and pressure in the Ideal Gas equation? |
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Definition
Inversely proportional:
Gas molecules have more space to move around in when volume increases, so they hit the container walls less frequently and pressure decreases. |
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Term
| What is the Ideal Gas equation (include units)? |
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Definition
| PV=nRT, where P=pressure in atm, V=volume in L, n=moles, R=constant of 0.08206 (L*atm)/(mol*K), and T=temperature in K (C+273.15) |
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Term
| 1 mole of any gas at STP occupies how much volume? |
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Definition
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Term
| Provide the ratios for partial pressure. |
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Definition
Moles of gas A : Total moles in container =
Partial pressure of gas A : Total pressure of container =
Volume of gas A at STP : 22.4 L |
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