Term
| Why are gases easier to compress than solids or liquids are? |
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Definition
| gases are easily compressed because of the space between the particles in a gas. |
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Term
| What are the three factors that affect gas pressure? |
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Definition
| the amount of gas, volume, and temperature are factors that affect gas pressure. |
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Definition
| a measure of how much the volume of matter decreases under pressure. |
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Term
| How are the pressure, volume, and temperature of a gas related? |
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Definition
| if a temperature is constant, as the pressure of a gas increases, the volume decreases. As the temperature of an enclosed gas increases, the volume increases, if the pressure is constant. As the temperature of an enclosed gas increases, the pressure increases, if the volume is constant. |
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Term
| When is the combined gas law used to solve problems? |
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Definition
| the combined gas law allows you to do calculations for situations in which only the amount of gas is constant. |
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Term
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Definition
| states that for a given mass of gas at constant temperature, the volume of the gas varies inversely with pressure. |
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Term
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Definition
| states that the colume of a fixed mass of gas is directly proportional to its Kelvin temperature if the pressure is kept constant. |
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Definition
| states that the pressure of a gas is directly proportional to the Kelvin temperature if the volume remains constant. |
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Term
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Definition
| describes the relationship among the pressure, temperature, and volume of an enclosed gas. |
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Term
| What is needed to calculate the amount of gas in a sample at given conditions of volume, temperature, and pressure? |
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Definition
| to calculate the number of moles of a contained gas requires an expression that contains the variable n. |
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Term
| Under what conditions are real gases most likely to differ from ideal gases? |
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Definition
| real gases differ most from an ideal gas at low temperatures and high pressures. |
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Term
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Definition
| (R) has the value 8.31 (L*kPa)/(K*mol). |
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Term
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Definition
| includes all four variables--P,V,T,and n. Usually written PV=nRT. |
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Term
| How is the total pressure of a mixture of gases related to the partial pressure of the component gases? |
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Definition
| in a mixture of gases, the total pressure is the sum of the partial pressure of the gases. |
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Term
| How does the molar mass of a gas affect the rate at which the gas effuses or diffuses? |
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Definition
| gases of lower molar mass diffuse and effuse faster than gases of higher molar mass. |
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Term
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Definition
| the contribution each gas in a mixture makes to the total pressure. |
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Term
| Dalton's law of partial pressures |
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Definition
| states that, at constant volume and temperature, the total pressure exerted by a mixture of gases is equal to the sum of the partial pressures of the component gases. |
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Term
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Definition
| the tendency of molecules to move toward areas of lower concentration until the concentration is uniform throughout. |
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Term
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Definition
| a gas escapes through a tiny hole in its container. |
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Term
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Definition
| states that the rate of effusion of a gas is inversely proportional to the square root of the gas's molar mass. |
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