Gas Laws Flipbook

Gas Laws Flipbook Drishita Koya

Properties of Gases Kinetic Molecular Theory Only 4 quantities are required in order to define the state of gas: 1. The quantity of gas, n (moles) 2. The temperature of the gas, T (in Kelvins) 3. The volume of the gas, V (liters) 4. The pressure of the gas, P (atmosphere) https://www.google.com/search?q=kinetic+molecular+theory&sxsrf=ALeKk03T_WCSNO39FNpPLZEpiA-iLxFsqg:1621226308889&source=lnms&tbm=isch&sa=X&ved=2ahUKEwjj-vbR8s_wAhVILs0KHSrDAgkQ_AUoAXoECAEQAw&biw=1066&bih=889#imgrc=sYKB7e_3Da3TNM&imgdii=TvnQUK0l6bjbNM

Volume, Temperature, and Pressure Volume: i: Definition: the amount of space a substance occupies. Volume is dependent on the 3 quantities: length, width, and height. ii: Units: Liters (L) iii: Conversion Methods: Length * Base * Height = Volume Temperature: i: Definition: Temperature is proportional to the average random kinetic energy of ideal gases. The degree of hotness or coldness of a body or environment (corresponding to its molecular theory). ii: Units: Celsius and Kelvin scale iii: Conversion Methods: F = 9/5 + 32 & K = C + 273 Pressure: i: Definition: Pressure refers to the number of collisions that gas particles have with their container and/or surroundings. ii: Units: P (atmosphere) iii: Conversion Methods: The Standard Atmospheric Pressure = 1 atm = 760.00 mmHg = 760.00 torr = 29.92 Hg = 14.7 psi = 101.325 kPa = 10^5 Pa https://www.google.com/search?q=properties+of+gases&sxsrf=ALeKk00ncBYeGGK7-60S9mycZQ_xaV-k9A:1621259132180&source=lnms&tbm=isch&sa=X&ved=2ahUKEwi-4aX17NDwAhUPqJ4KHXLHDO4Q_AUoAXoECAEQAw&biw=1056&bih=946#imgrc=FUzKHwht7cQ7-M

Ideal Gas Law Ideal Gas Law The Ideal Gas Law is the gas behavior that permits an individual to solve for the number of moles of a contained gas when given only 1 value for each P,V, and T. Variables that are related in this law would be the pressure (low) and the temperature (high) which create ideal conditions in which the Ideal Gases can exist. Constant variables in the law would be: 0.0821 L * atm/mol * K 62.4 L * mmHg/mol * K 8.314 L * kPa/mol * K The formula for the Ideal Gas Law is PV = nRT https://www.google.com/search?q=ideal+gas+law+pic&tbm=isch&ved=2ahUKEwjxw6rF8M_wAhXD41MKHXI4CHsQ2-cCegQIABAA&oq=ideal+gas+law+pic&gs_lcp=CgNpbWcQAzICCAA6BAgAEEM6BAgAEBhQ_iZY6ylggStoAHAAeACAAUiIAYUCkgEBNJgBAKABAaoBC2d3cy13aXotaW1nwAEB&sclient=img&ei=EfGhYLH3I8PHzwLy8KDYBw&bih=889&biw= 857#imgrc=QPEPcMGbThrBAM

Avogadro’s Principle/Molar Volume The molar volume is the volume that one mole of gas occupies at STP or 22.4 L. The conversion factor for this molar volume is 22.4 L = 1 mol at STP. STP stands for the standard temperature (273 K or at 0 degrees C) and standard pressure (101.3 kPa or 1 atm). https://www.google.com/search?q=avogadro%27s+principle&sxsrf=ALeKk004IW85hCzIg0BrDrgA-9ffdzrUdw:1621226092013&source=lnms&tbm=isch&sa=X&ved=2ahUKEwjOh8Lq8c_wAhX0B50JHejlCacQ_AUoAXoECAEQAw&biw=1066&bih=946&dpr=2#imgrc=7lFoldR17uC9UM

Experimental Gas Laws Boyle's Law: The law states that the volume of a confined gas is inversely proportional to the pressure exerted on the gas. The variables related in the law would be volume, temperature, and pressure, where volume and pressure are inversely proportional. This means that as the pressure increases, the volume will decrease. This could also happen in the opposite manner, with volume increasing, pressure decreasing. The variables that are constant would be the volume and the pressure; They are at constant temperature. However, one thing to note is that this law only holds true at low pressures. The easiest form to memorize in Boyle’s Laws would be P1V1 = P2V2 https://www.google.com/search?q=boyle%27s+law&sxsrf=ALeKk02C8zwmQgXRy1KvLTXl1EvBT-7UiQ:1621220544845&source=lnms&tbm=isch&sa=X&ved=2ahUKEwjeybWV3c_wAhXaPM0KHcnjC1EQ_AUoAXoECAEQAw&biw=1525&bih=946#imgrc=i4QNd4JlYltnzM

Charles Law: If a given quantity of gas is held at a constant pressure, then its volume is directly proportional to the absolute pressure. However, you must use Kelvins. In this law, temperature and volume are the variables that are considered related. For example, temperature and volume are at constant temperature. This could mean as the temperature increases, the volume also increases and vice versa. A constant variable in Charles’s law would be pressure because it is meant to be constant for temperature to stay proportional to the volume. The formula for Charles Law is (in simple terms) V1/T1 = V2/T2 https://www.google.com/search?q=charles+law&sxsrf=ALeKk0325xivwJY8UdhVMgopVNXOc0_dTA:1621223822144&source=lnms&tbm=isch&sa=X&ved=2ahUKEwiIkpSw6c_wAhXKGs0KHbycBpUQ_AUoAXoECAEQAw&biw=1525&bih=946#imgrc=UTDRYYPaobWjPM

Gay-Lussac’s Law Volumes of gases always combine with one another in the ratio of small whole numbers as long as whole numbers are measured at the same temperature and pressure. At a constant volume, temperature and pressure are directly related to one another. A constant variable in Gay-Lussac’s Law would be volume because when pressure increases, so does temperature and vice versa. This is assuming that the container is not expandable. The formula used in Gay-Lussac’s Law can be written as P1/T2 = P2/T2 When you increase the temperature, the kinetic energy is also increased, which is then increasing the number of collisions. This then leads to the increase of pressure in the container. https://www.google.com/search?q=gay-lussac%27s+law&sxsrf=ALeKk00RTqqfF7qA34kubgjslLnkktAePA:1621224663670&source=lnms&tbm=isch&sa=X&ved=2ahUKEwiogLfB7M_wAhUOQ80KHWKQDqEQ_AUoAXoECAEQAw&biw=1525&bih=902#imgrc=-DPZkNo88R4LgM&imgdii=Zruz3KHEYNAVcM

Combined Gas Law The Combined Gas Law combines the Laws of Boyle, Charles, and Gay-Lussac; in this, you can use this law to to find the equations to all of the other laws. In this law, the relationship between temperature, pressure, and volume is expressed with a fixed amount of gas. The amount of gas is the only common constant variable in the Combined Gas Law. The formula for this law is (P1 * V1)/T1 = (P2 * V2)/T2 https://www.google.com/search?q=combined+gas+law&sxsrf=ALeKk03FKuTXqGIdR-dZLC1VUkhR5ftZ6w:1621225234643&source=lnms&tbm=isch&sa=X&ved=2ahUKEwiMqdjR7s_wAhXEHM0KHYDtA2wQ_AUoAXoECAEQAw&biw=1525&bih=946#imgrc=4WLkupg2o2U_iM&imgdii=QzkbVrbOgypsiM

Practice Problems a) A fixed volume steel tank holds 50.0 L of oxygen gas at 10.0oC and 2.0 atm. What will the pressure in the tank be if it is moved to a room that has a temperature of 25.0oC? b) A helium filled weather balloon has a volume of 25.0 L at 23.0oC and 0.963 atm when it is released from the weather station. In the upper atmosphere at a location where the pressure is 0.584 atm, the balloon increases to 34.7 L. What is the Celsius temperature of the balloon at the higher altitude? c) In a double replacement reaction, 5.00 moles of water vapor are produced at 760 mmHg and 300 K. What volume of water will be collected?

d) A cylinder is filled to a volume of 3.50 L at 760 mmHg with chlorine gas. What is the volume if the pressure is changed to 50.0 kPa? e) How many moles argon gas are found when 2.3 L are isolated from a sample of air at STP? How many grams of argon are in the container? f) A gas originally occupies an unknown volume at 27 oC. It currently occupies 40.0 mL at -123oC. What was the original volume?

g) Using dimensional analysis: Convert 23 kPa to mmHg and then to atmospheres. h) Convert 100 K to Celsius. Convert 100 oC to Kelvin. i) Using dimensional analysis: Convert 150 mL to liters. Convert 3.00 L to mL. j) At STP, a sample of methane gas (CH4) is combusted to produce 1.2 L carbon dioxide. What volume of oxygen was required for the reaction to occur?