Gas Laws Purpose of the Experiment To demonstrate
![*Gas Laws* Purpose of the Experiment To demonstrate the complexities involved in measuring properties *Gas Laws* Purpose of the Experiment To demonstrate the complexities involved in measuring properties](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-1.jpg)
![Physical Characteristics of Gases Physical Characteristics Volume, V Typical Units liters (L) Pressure, P Physical Characteristics of Gases Physical Characteristics Volume, V Typical Units liters (L) Pressure, P](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-2.jpg)
![Boyle’s Law Pressure and volume are inversely related at constant temperature. PV = K Boyle’s Law Pressure and volume are inversely related at constant temperature. PV = K](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-3.jpg)
![Boyle’s Law: P 1 V 1 = P 2 V 2 Boyle’s Law: P 1 V 1 = P 2 V 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-4.jpg)
![Boyle’s Law: P 1 V 1 = P 2 V 2 Boyle’s Law: P 1 V 1 = P 2 V 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-5.jpg)
![Charles’ Law Volume of a gas varies directly with the absolute temperature at constant Charles’ Law Volume of a gas varies directly with the absolute temperature at constant](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-6.jpg)
![Charles’ Law: V 1/T 1 = V 2/T 2 Charles’ Law: V 1/T 1 = V 2/T 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-7.jpg)
![Charles’ Law: V 1/T 1 = V 2/T 2 Charles’ Law: V 1/T 1 = V 2/T 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-8.jpg)
![Avogadro’s Law At constant temperature and pressure, the volume of a gas is directly Avogadro’s Law At constant temperature and pressure, the volume of a gas is directly](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-9.jpg)
![Avogadro’s Law: V 1/n 1=V 2/n 2 Avogadro’s Law: V 1/n 1=V 2/n 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-10.jpg)
![Gay-Lussac Law At constant volume, pressure and absolute temperature are directly related. P = Gay-Lussac Law At constant volume, pressure and absolute temperature are directly related. P =](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-11.jpg)
![Dalton’s Law The total pressure in a container is the sum of the pressure Dalton’s Law The total pressure in a container is the sum of the pressure](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-12.jpg)
![Dalton’s Law Dalton’s Law](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-13.jpg)
![Vapor Pressure Water evaporates! When that water evaporates, the vapor has a pressure. Gases Vapor Pressure Water evaporates! When that water evaporates, the vapor has a pressure. Gases](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-14.jpg)
![Differences Between Ideal and Real Gases Ideal Gas Real Gas Always Only at very Differences Between Ideal and Real Gases Ideal Gas Real Gas Always Only at very](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-15.jpg)
![Real Gases Real molecules do take up space and do interact with each other Real Gases Real molecules do take up space and do interact with each other](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-16.jpg)
![Ideally, the VOLUME of the molecules was neglected: Ar gas, ~to scale, in a Ideally, the VOLUME of the molecules was neglected: Ar gas, ~to scale, in a](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-17.jpg)
![But since real gases do have volume, we need: Volume Correction The actual volume But since real gases do have volume, we need: Volume Correction The actual volume](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-18.jpg)
![Pressure Correction Because the molecules are attracted to each other, the pressure on the Pressure Correction Because the molecules are attracted to each other, the pressure on the](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-19.jpg)
![Van der Waal’s equation Corrected Pressure Corrected Volume “a” and “b” are determined by Van der Waal’s equation Corrected Pressure Corrected Volume “a” and “b” are determined by](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-20.jpg)
![Compressibility Factor The most useful way of displaying this new law for real molecules Compressibility Factor The most useful way of displaying this new law for real molecules](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-21.jpg)
![Part 1: Molar Volume of Butane Page 194 -195 in your Lab Packet If Part 1: Molar Volume of Butane Page 194 -195 in your Lab Packet If](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-22.jpg)
![Molar mass of butane (C 4 H 10) = _____ g/mole Mass of butane: Molar mass of butane (C 4 H 10) = _____ g/mole Mass of butane:](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-23.jpg)
![Molar mass of butane (C 4 H 10) = _____ g/mole (12. 011 4) Molar mass of butane (C 4 H 10) = _____ g/mole (12. 011 4)](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-24.jpg)
![Ask your TA for the Lab Temperature and Pressure* T = ____ o. C Ask your TA for the Lab Temperature and Pressure* T = ____ o. C](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-25.jpg)
![Apparent molar volume of butane at STP; Vm = _____L/mole Lab pressure 0. 500 Apparent molar volume of butane at STP; Vm = _____L/mole Lab pressure 0. 500](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-26.jpg)
![Partial pressure of water vapor in flask: Pw = ______torr calculate x Lab temperature Partial pressure of water vapor in flask: Pw = ______torr calculate x Lab temperature](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-27.jpg)
![Partial pressure of butane in flask: _____ torr _____atm calculate PB = Ptotal -Pw Partial pressure of butane in flask: _____ torr _____atm calculate PB = Ptotal -Pw](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-28.jpg)
![Partial pressure of butane: Pvdw = ____ atm 0. 08206 L. atm/mole. K Already Partial pressure of butane: Pvdw = ____ atm 0. 08206 L. atm/mole. K Already](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-29.jpg)
![Compressibility factor for butane : ZB = ____ Partial pressure of butane in flask Compressibility factor for butane : ZB = ____ Partial pressure of butane in flask](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-30.jpg)
![Estimated second Virial Coefficient for Butane at room temperature: BB = ______L/mole 0. 500 Estimated second Virial Coefficient for Butane at room temperature: BB = ______L/mole 0. 500](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-31.jpg)
![Part 2: Buoyancy Effect Filling Ziplok bag with butane gas Page 197 in your Part 2: Buoyancy Effect Filling Ziplok bag with butane gas Page 197 in your](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-32.jpg)
![Initial mass cartridge____g bag _____ g Final mass ____g _____g Change in mass ____g Initial mass cartridge____g bag _____ g Final mass ____g _____g Change in mass ____g](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-33.jpg)
![Calculated volume of Butane in bag: ____L Calculated in previous step calculate Estimated second Calculated volume of Butane in bag: ____L Calculated in previous step calculate Estimated second](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-34.jpg)
![Estimated density of air at experimental T and P: d= ____g / L Buoyancy Estimated density of air at experimental T and P: d= ____g / L Buoyancy](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-35.jpg)
![Estimated Molar mass of air: _____g/mole Estimated density of air (calculated in previous step) Estimated Molar mass of air: _____g/mole Estimated density of air (calculated in previous step)](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-36.jpg)
![Part 3: Conservation of Mass Gas generating reaction in a closed system Page 199 Part 3: Conservation of Mass Gas generating reaction in a closed system Page 199](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-37.jpg)
![Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-38.jpg)
![Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-39.jpg)
![Weight of bag and reaction components: Before reaction: _____ g after reaction : ______ Weight of bag and reaction components: Before reaction: _____ g after reaction : ______](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-40.jpg)
![Reaction: 1 Na. HCO 3(aq) + CH 3 CO 2 H(aq) _____ + 1 Reaction: 1 Na. HCO 3(aq) + CH 3 CO 2 H(aq) _____ + 1](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-41.jpg)
![Check Out from the Stockroom 1000 ml beaker 500 ml volumetric flask Tygon tubing Check Out from the Stockroom 1000 ml beaker 500 ml volumetric flask Tygon tubing](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-42.jpg)
![This Week: April 28 - 30 Turn In: Gas Laws Experiment pp. 195 -199 This Week: April 28 - 30 Turn In: Gas Laws Experiment pp. 195 -199](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-43.jpg)
![Chem 1319 Final Exam – May 5 - 7 1 Hour Exam during regularly Chem 1319 Final Exam – May 5 - 7 1 Hour Exam during regularly](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-44.jpg)
![* *It’s a biology joke! Don’t be a dumb bunny! - Study! * *It’s a biology joke! Don’t be a dumb bunny! - Study!](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-45.jpg)
- Slides: 45
![Gas Laws Purpose of the Experiment To demonstrate the complexities involved in measuring properties *Gas Laws* Purpose of the Experiment To demonstrate the complexities involved in measuring properties](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-1.jpg)
*Gas Laws* Purpose of the Experiment To demonstrate the complexities involved in measuring properties of gases related to: 1. ) Complications in weighing due to the buoyancy of air; 2. ) Problems in pressure measurements over water; and, 3. ) Non-ideality of Gases.
![Physical Characteristics of Gases Physical Characteristics Volume V Typical Units liters L Pressure P Physical Characteristics of Gases Physical Characteristics Volume, V Typical Units liters (L) Pressure, P](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-2.jpg)
Physical Characteristics of Gases Physical Characteristics Volume, V Typical Units liters (L) Pressure, P Temperature, T atmosphere (1 atm = 1. 015 x 105 N/m 2) Kelvin (K) Number of atoms or molecules, n mole (1 mol = 6. 022 x 1023 atoms or molecules)
![Boyles Law Pressure and volume are inversely related at constant temperature PV K Boyle’s Law Pressure and volume are inversely related at constant temperature. PV = K](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-3.jpg)
Boyle’s Law Pressure and volume are inversely related at constant temperature. PV = K As one goes up, the other goes down. P 1 V 1 = P 2 V 2 “Father of Modern Chemistry” Robert Boyle Chemist & Natural Philosopher Listmore, Ireland January 25, 1627 – December 30, 1690
![Boyles Law P 1 V 1 P 2 V 2 Boyle’s Law: P 1 V 1 = P 2 V 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-4.jpg)
Boyle’s Law: P 1 V 1 = P 2 V 2
![Boyles Law P 1 V 1 P 2 V 2 Boyle’s Law: P 1 V 1 = P 2 V 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-5.jpg)
Boyle’s Law: P 1 V 1 = P 2 V 2
![Charles Law Volume of a gas varies directly with the absolute temperature at constant Charles’ Law Volume of a gas varies directly with the absolute temperature at constant](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-6.jpg)
Charles’ Law Volume of a gas varies directly with the absolute temperature at constant pressure. V = KT V 1 / T 1 = V 2 / T 2 Jacques-Alexandre Charles Mathematician, Physicist, Inventor Beaugency, France November 12, 1746 – April 7, 1823
![Charles Law V 1T 1 V 2T 2 Charles’ Law: V 1/T 1 = V 2/T 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-7.jpg)
Charles’ Law: V 1/T 1 = V 2/T 2
![Charles Law V 1T 1 V 2T 2 Charles’ Law: V 1/T 1 = V 2/T 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-8.jpg)
Charles’ Law: V 1/T 1 = V 2/T 2
![Avogadros Law At constant temperature and pressure the volume of a gas is directly Avogadro’s Law At constant temperature and pressure, the volume of a gas is directly](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-9.jpg)
Avogadro’s Law At constant temperature and pressure, the volume of a gas is directly related to the number of moles. V = K n V 1 / n 1 = V 2 / n 2 Amedeo Avogadro Physicist Turin, Italy August 9, 1776 – July 9, 1856
![Avogadros Law V 1n 1V 2n 2 Avogadro’s Law: V 1/n 1=V 2/n 2](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-10.jpg)
Avogadro’s Law: V 1/n 1=V 2/n 2
![GayLussac Law At constant volume pressure and absolute temperature are directly related P Gay-Lussac Law At constant volume, pressure and absolute temperature are directly related. P =](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-11.jpg)
Gay-Lussac Law At constant volume, pressure and absolute temperature are directly related. P = k T P 1 / T 1 = P 2 / T 2 Joseph-Louis Gay-Lussac Experimentalist Limoges, France December 6, 1778 – May 9, 1850
![Daltons Law The total pressure in a container is the sum of the pressure Dalton’s Law The total pressure in a container is the sum of the pressure](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-12.jpg)
Dalton’s Law The total pressure in a container is the sum of the pressure each gas would exert if it were alone in the container. The total pressure is the sum of the partial pressures. PTotal = P 1 + P 2 + P 3 + P 4 + P 5. . . (For each gas P = n. RT/V) John Dalton Chemist & Physicist Eaglesfield, Cumberland, England September 6, 1766 – July 27, 1844
![Daltons Law Dalton’s Law](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-13.jpg)
Dalton’s Law
![Vapor Pressure Water evaporates When that water evaporates the vapor has a pressure Gases Vapor Pressure Water evaporates! When that water evaporates, the vapor has a pressure. Gases](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-14.jpg)
Vapor Pressure Water evaporates! When that water evaporates, the vapor has a pressure. Gases are often collected over water so the vapor pressure of water must be subtracted from the total pressure.
![Differences Between Ideal and Real Gases Ideal Gas Real Gas Always Only at very Differences Between Ideal and Real Gases Ideal Gas Real Gas Always Only at very](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-15.jpg)
Differences Between Ideal and Real Gases Ideal Gas Real Gas Always Only at very low P and high T Molecular volume Zero Small but nonzero Molecular attractions Zero Small Molecular repulsions Zero Small Obey PV=n. RT
![Real Gases Real molecules do take up space and do interact with each other Real Gases Real molecules do take up space and do interact with each other](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-16.jpg)
Real Gases Real molecules do take up space and do interact with each other (especially polar molecules). Need to add correction factors to the ideal gas law to account for these.
![Ideally the VOLUME of the molecules was neglected Ar gas to scale in a Ideally, the VOLUME of the molecules was neglected: Ar gas, ~to scale, in a](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-17.jpg)
Ideally, the VOLUME of the molecules was neglected: Ar gas, ~to scale, in a box 3 nm at 1 Atmosphere Pressure at 10 Atmospheres Pressure at 30 Atmospheres Pressure
![But since real gases do have volume we need Volume Correction The actual volume But since real gases do have volume, we need: Volume Correction The actual volume](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-18.jpg)
But since real gases do have volume, we need: Volume Correction The actual volume free to move in is less because of particle size. More molecules will have more effect. Corrected volume V’ = V – nb “b” is a constant that differs for each gas.
![Pressure Correction Because the molecules are attracted to each other the pressure on the Pressure Correction Because the molecules are attracted to each other, the pressure on the](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-19.jpg)
Pressure Correction Because the molecules are attracted to each other, the pressure on the container will be less than ideal. Pressure depends on the number of molecules per liter. Since two molecules interact, the effect must be squared.
![Van der Waals equation Corrected Pressure Corrected Volume a and b are determined by Van der Waal’s equation Corrected Pressure Corrected Volume “a” and “b” are determined by](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-20.jpg)
Van der Waal’s equation Corrected Pressure Corrected Volume “a” and “b” are determined by experiment “a” and “b” are different for each gas bigger molecules have larger “b” “a” depends on both size and polarity Johannes Diderik van der Waals Mathematician & Physicist Leyden, The Netherlands November 23, 1837 – March 8, 1923
![Compressibility Factor The most useful way of displaying this new law for real molecules Compressibility Factor The most useful way of displaying this new law for real molecules](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-21.jpg)
Compressibility Factor The most useful way of displaying this new law for real molecules is to plot the compressibility factor, Z : For n = 1 Z = PV / RT Ideal Gases have Z = 1
![Part 1 Molar Volume of Butane Page 194 195 in your Lab Packet If Part 1: Molar Volume of Butane Page 194 -195 in your Lab Packet If](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-22.jpg)
Part 1: Molar Volume of Butane Page 194 -195 in your Lab Packet If you would like to take notes, these slides start on page 201 of your Lab Packet.
![Molar mass of butane C 4 H 10 gmole Mass of butane Molar mass of butane (C 4 H 10) = _____ g/mole Mass of butane:](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-23.jpg)
Molar mass of butane (C 4 H 10) = _____ g/mole Mass of butane: _____ n or n. B= _______
![Molar mass of butane C 4 H 10 gmole 12 011 4 Molar mass of butane (C 4 H 10) = _____ g/mole (12. 011 4)](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-24.jpg)
Molar mass of butane (C 4 H 10) = _____ g/mole (12. 011 4) + (1. 008 10) = 58. 124 Mass of butane: _____ Initial weight of cartridge – final weight of cartridge n or n. B= _______
![Ask your TA for the Lab Temperature and Pressure T o C Ask your TA for the Lab Temperature and Pressure* T = ____ o. C](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-25.jpg)
Ask your TA for the Lab Temperature and Pressure* T = ____ o. C P = _____torr V = _____L T = ____ K P = _____atm 0. 500 L Note: K = o. C + 273. 15 & 1 atm = 760 torr Apparent molar volume, (Vm = V / n) of butane at experimental T & P: 0. 500 L Vm = ____ L / mole V/n n → Calculated earlier *These will be posted on the chalkboard. Verify the values are for your session before recording in your book.
![Apparent molar volume of butane at STP Vm Lmole Lab pressure 0 500 Apparent molar volume of butane at STP; Vm = _____L/mole Lab pressure 0. 500](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-26.jpg)
Apparent molar volume of butane at STP; Vm = _____L/mole Lab pressure 0. 500 L 1 atm or 760 torr calculate Lab temperature (K) calculate 273. 15 K V 2 Already calculated
![Partial pressure of water vapor in flask Pw torr calculate x Lab temperature Partial pressure of water vapor in flask: Pw = ______torr calculate x Lab temperature](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-27.jpg)
Partial pressure of water vapor in flask: Pw = ______torr calculate x Lab temperature (K)
![Partial pressure of butane in flask torr atm calculate PB Ptotal Pw Partial pressure of butane in flask: _____ torr _____atm calculate PB = Ptotal -Pw](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-28.jpg)
Partial pressure of butane in flask: _____ torr _____atm calculate PB = Ptotal -Pw Lab pressure (torr) calculated in previous step (torr)
![Partial pressure of butane Pvdw atm 0 08206 L atmmole K Already Partial pressure of butane: Pvdw = ____ atm 0. 08206 L. atm/mole. K Already](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-29.jpg)
Partial pressure of butane: Pvdw = ____ atm 0. 08206 L. atm/mole. K Already calculated Lab temp. 14. 47 atm. L 2/mole 2 calculate 0. 500 L 0. 1226 L/mole
![Compressibility factor for butane ZB Partial pressure of butane in flask Compressibility factor for butane : ZB = ____ Partial pressure of butane in flask](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-30.jpg)
Compressibility factor for butane : ZB = ____ Partial pressure of butane in flask (atm) Calculated earlier 0. 500 L calculate same as “n” already calculated Lab temperature (K) 0. 08206 L. atm/mole. K
![Estimated second Virial Coefficient for Butane at room temperature BB Lmole 0 500 Estimated second Virial Coefficient for Butane at room temperature: BB = ______L/mole 0. 500](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-31.jpg)
Estimated second Virial Coefficient for Butane at room temperature: BB = ______L/mole 0. 500 L calculate already calculated Calculated in previous step Compressibility factor for butane
![Part 2 Buoyancy Effect Filling Ziplok bag with butane gas Page 197 in your Part 2: Buoyancy Effect Filling Ziplok bag with butane gas Page 197 in your](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-32.jpg)
Part 2: Buoyancy Effect Filling Ziplok bag with butane gas Page 197 in your Lab Packet
![Initial mass cartridgeg bag g Final mass g g Change in mass g Initial mass cartridge____g bag _____ g Final mass ____g _____g Change in mass ____g](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-33.jpg)
Initial mass cartridge____g bag _____ g Final mass ____g _____g Change in mass ____g _____g Discrepancy is the difference between these two masses Discrepancy: _____g Moles of Butane in bag: n = _____ moles Change in cartridge mass calculate 58. 124 g/mole
![Calculated volume of Butane in bag L Calculated in previous step calculate Estimated second Calculated volume of Butane in bag: ____L Calculated in previous step calculate Estimated second](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-34.jpg)
Calculated volume of Butane in bag: ____L Calculated in previous step calculate Estimated second Virial Coefficient for Butane at room temperature Calculated in Part 1 (p 195). Compressibility factor for Butane Calculated in Part 1 (p 195).
![Estimated density of air at experimental T and P d g L Buoyancy Estimated density of air at experimental T and P: d= ____g / L Buoyancy](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-35.jpg)
Estimated density of air at experimental T and P: d= ____g / L Buoyancy effect of displaced volume of air (the mass discrepancy) calculate Calculated volume of Butane in bag (calculated in previous step)
![Estimated Molar mass of air gmole Estimated density of air calculated in previous step Estimated Molar mass of air: _____g/mole Estimated density of air (calculated in previous step)](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-36.jpg)
Estimated Molar mass of air: _____g/mole Estimated density of air (calculated in previous step) 0. 08206 L. atm/mole. K Lab temperature (K) calculate Lab pressure (atm)
![Part 3 Conservation of Mass Gas generating reaction in a closed system Page 199 Part 3: Conservation of Mass Gas generating reaction in a closed system Page 199](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-37.jpg)
Part 3: Conservation of Mass Gas generating reaction in a closed system Page 199 in your Lab Packet
![Part 3 Conservation of Mass Gas generating reaction in a closed system Molar mass Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-38.jpg)
Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass of Na. HCO 3 : _____g/mole Moles of Na. HCO 3: _______ mole
![Part 3 Conservation of Mass Gas generating reaction in a closed system Molar mass Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-39.jpg)
Part 3: Conservation of Mass Gas generating reaction in a closed system Molar mass of Na. HCO 3 : _____g/mole (22. 990) + (1. 008) + (12. 011) + (3 15. 999) = 84. 006 g/mole Moles of Na. HCO 3: _______ mole
![Weight of bag and reaction components Before reaction g after reaction Weight of bag and reaction components: Before reaction: _____ g after reaction : ______](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-40.jpg)
Weight of bag and reaction components: Before reaction: _____ g after reaction : ______ g Discrepancy is the difference between these two weights. Discrepancy: _____g Estimated volume of expansion: _______ L calculate Determined in Part 2 (p 197).
![Reaction 1 Na HCO 3aq CH 3 CO 2 Haq 1 Reaction: 1 Na. HCO 3(aq) + CH 3 CO 2 H(aq) _____ + 1](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-41.jpg)
Reaction: 1 Na. HCO 3(aq) + CH 3 CO 2 H(aq) _____ + 1 CO 2(g) + ______ Expected moles of CO 2(gas) : ______ moles Expected volume of gas at laboratory T & P: _____L 0. 08206 L. atm/mole. K Expected moles of CO 2 (from previous step) calculate Lab temp. (K) Lab pressure (atm) Partial pressure of water vapor. (Note: Convert your Pw to atm. ) (You calculated Pw in torr in Part 1 – p 195. )
![Check Out from the Stockroom 1000 ml beaker 500 ml volumetric flask Tygon tubing Check Out from the Stockroom 1000 ml beaker 500 ml volumetric flask Tygon tubing](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-42.jpg)
Check Out from the Stockroom 1000 ml beaker 500 ml volumetric flask Tygon tubing with Hook Butane cylinder 1 piece of plastic wrap 1 quart Ziploc Bag 5 dram vial with lid* In The Hood: 50% Acetic Acid in a 500 ml plastic dispenser By Balances: Sodium bicarbonate, Na. HCO 3 Clean Up: *Dispose of liquid waste in appropriate container. Rinse vial and lid with water and return them to the stockroom. Hazards: 50% Acetic acid (corrosive, sharp, irritating odor) Butane (flammable) Waste: 5 gallon liquid waste for Na. HCO 3 and acetic acid
![This Week April 28 30 Turn In Gas Laws Experiment pp 195 199 This Week: April 28 - 30 Turn In: Gas Laws Experiment pp. 195 -199](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-43.jpg)
This Week: April 28 - 30 Turn In: Gas Laws Experiment pp. 195 -199 + calculations page. The r e is Students must do all calculations before leaving lab, no Pos tlab due to the complex nature of the calculations. ! Calculations must be shown on a separate piece of paper, with units to the correct number of significant figures. Datasheets need to be in ink, but calculations may be done with pen or pencil. Calculations scribbled in the margins of the lab pages are NOT ACCEPTABLE. Evaluation Forms: To evaluate Chem 1319, you should be receiving an email from the CET Committee with the following link: https: //itweb. mst. edu/auth-cgi-bin/cgiwrap/distanceed/evals/survey. pl The Chemistry Outstanding TA Awards are based on these evaluations. So please complete the evaluations, as TAs without enough surveys completed are not considered eligible for the award.
![Chem 1319 Final Exam May 5 7 1 Hour Exam during regularly Chem 1319 Final Exam – May 5 - 7 1 Hour Exam during regularly](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-44.jpg)
Chem 1319 Final Exam – May 5 - 7 1 Hour Exam during regularly scheduled class time*. You will need a calculator. Checkout after exam. ($35 fine for not checking out. ) Verify all of the equipment is in the drawer. Fill in green slips for any broken items. (This means NO Chem 1319 Final during Finals Week. ) *If you need to take the test on a different day, email Dr. Bolon. If you are taking the test at the testing center, email Dr. Bolon. Review Session – Tuesday, April 28, 4: 00 pm – 6: 00 pm in G 3 Schrenk.
![Its a biology joke Dont be a dumb bunny Study * *It’s a biology joke! Don’t be a dumb bunny! - Study!](https://slidetodoc.com/presentation_image/441366c2c93daa1e098ca4432064ac5b/image-45.jpg)
* *It’s a biology joke! Don’t be a dumb bunny! - Study!
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