AP Chemistry - Chandler Unified School District
|Concepts |Details |
|What is pressure? |A. Properties of Gases |
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| |B. Measuring Barometric Pressure |
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|Pressure conversions | |
| |The pressure of a gas is measure as 49 torr. Represent this pressure in both atmospheres and pascals. |
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|The Gas Laws of Boyle, |Boyle’s Law |
|Charles and Avagadro | |
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| |Charles Law |
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| |Avagadro’s Law |
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| |Sulfur Dioxide, a gas that plays a central role in the formations of acid rain, is found in the exhaust|
| |of automobiles and power plants. Consider a 1.53 Liter sample of gaseous SO2 at a pressure of 5.6 x |
| |103 Pa at a constant temperature, If the pressure is changed to 1.5 x 104 Pa, what will be the new |
| |volume of the gas? |
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| |A sample of gas at 15(C and 1 atm has a volume of 2.58 L. What volume will this gas occupy at 38(C and|
| |1 atm? |
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| |Suppose we have a 12.2-liter sample containing 0.50-mol oxygen gas at a pressure of 1 atm and a |
| |temperature of 25(C. If all this O2 were converted to ozone (O3) at the same temp and pressure, what |
| |would be the volume of ozone? |
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|Ideal Gas Law |Derivation from existing Laws |
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| |Limitations of the Ideal Gas Law |
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| |Solving for new volume, temp or pressure |
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|Ideal Gas Law Practice |A sample of Hydrogen gas (H2) has a volume of 8.56 L at a temperature of 0°C and a pressure of 1.5 atm.|
| |Calculate the moles of H2 molecules present in this gas sample. |
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| |Suppose we have a sample of ammonia gas with a volume of 3.5 L at a pressure of 1.68 atm. The gas is |
| |compressed to a volume of 1.35 L at a constant temperature. Use the ideal gas law to calculate the |
| |final pressure. |
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|More Ideal Gas Law |A sample of methane gas that has a volume of 3.8 L at 5°C is heated to 86°C at constant pressure. |
| |Calculate it’s new volume. |
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| |A sample of diborane gas (B2H6), a substance that bursts into flame when exposed to air, has a pressure|
| |of 345 torr at a temperature of -15°C and a volume of 3.48 L. If conditions are changed so that the |
| |temperature is 36°C and the pressure is 468 torr, what will the volume of the sample be? |
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|Gas Stoichiometry |Standard temperature and pressure (STP) |
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| |Molar Volume |
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| |Things to remember |
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|Practice |A sample of nitrogen gas has a volume of 1.75 L at STP. How many moles of N2 are present? |
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| |Quicklime (CaO) is produced by the thermal decomposition of calcium carbonate (CaCO3). Calculate the |
| |volume of CO2 at STP produced from the decomposition of 152 grams of CaCO3 by the reaction |
| |CaCO3(s) ( CaO(s) + CO2(g) |
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|Dalton’s Law of Partial |A. Statement of law |
|Pressures | |
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| |Mole Fraction |
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|Dalton’s Law Practice |Dalton’s Law 1 |
| |The partial pressure of oxygen was observed to be 156 torr in air with an atmospheric pressure of 743 |
| |torr. Calculate the mole fraction of O2 present. |
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| |Dalton’s Law 2 |
| |The mole fraction of nitrogen in the air is 0.7808. Calculate the partial pressure of N2 in air when |
| |the atmospheric pressure is 760 torr. |
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|The Kinetic Molecular |Postulates of the KMT Related to Ideal Gases |
|Theroy | |
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| |Explaining observed behavior with KMT (summarize each bullet, don’t copy word for word) |
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| |Root Mean Square Velocity |
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| |Mean Free Path |
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|Practice |Calculate the root mean square velocity for the atoms in a sample of helium gas (25(C). |
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| |Do all of the particles in a sample of gas at a constant temperature have the same velocity? Explain. |
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|Effusion and Diffusion |Effusion |
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| |Diffusion |
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|Effusion calculations |Calculate the ratio of the effusion rates of hydrogen gas and uranium hexafluoride (UF6), a gas used in|
| |the enrichment process to produce fuel for nuclear reactors. |
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|Real Gases |Ideal gases exist at ____________________ temp and _____________________pressure. |
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| |Real gases exist at ____________________ temp and _____________________pressure. |
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| |Why? |
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