(79) Cu)6.0-19) C6.6821)2?) 2.97 0.934 SL 3 A 9.) If 3 moles of a gas is in a 50ml gontainer at730 mmHg, What is the temperature of the gas? NS 5oml N2 T 2 \৭5 6 02462 O.9l0 Ta T2 if 10.) atmospheric pressure is 750mmHg and the vapor pressure of water is 45mmHg at 30°C? A gas is collected over water at 30°C. What is the pressure of the gas くレ

(79) Cu)6.0-19) C6.6821)2?) 2.97 0.934 SL 3 A 9.) If 3 moles of a gas is in a 50ml gontainer at730 mmHg, What is the temperature of the gas? NS 5oml N2 T 2 \৭5 6 02462 O.9l0 Ta T2 if 10.) atmospheric pressure is 750mmHg and the vapor pressure of water is 45mmHg at 30°C? A gas is collected over water at 30°C. What is the pressure of the gas くレ

Introduction to General, Organic and Biochemistry

11th Edition

ISBN:9781285869759

Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Publisher:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres

Chapter5: Gases, Liquids, And Solids

Section: Chapter Questions

Problem 5.24P

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5-54 Automobile air bags are inflated by nitrogen gas. When a significant collision occurs, an electronic sensor triggers the decomposition of sodium azide to form nitrogen gas and sodium metal. The nitrogen gas then inflates nylon bags, which protect the driver and front-seat passenger from impact with the dashboard and windshield. What volume of nitrogen gas measured at 1 atm and 27°C is formed by the decomposition of 100. g of sodium azide?
What is the value of FP for a sample of gas whose temperature is -33.0 C and volume is 0.0250 L? What temperature is required to change the volume to 66.9 cm3?
5-107 If 60.0 g of NH3 occupies 35.1 L under a pressure of 77.2 in. Hg, what is the temperature of the gas, in °C?
One type of gas mixture used in anesthesiologyis a 50%/50% mixture (by volume) of nitrous oxide (N2O) and oxygen(O2), which can be premixed and kept in a cylinder for later use.Because these two gases don’t react chemically at or below 2000 psi, attypical room temperatures they form a homogeneous single gas phase,which can be considered an ideal gas. If the temperature drops below-6C, however, N2O may begin to condense out of the gas phase. Thenany gas removed from the cylinder will initially be nearly pure O2; asthe cylinder empties, the proportion of O2 will decrease until the gascoming from the cylinder is nearly pure N2O. In a hospital, pure oxygen may be delivered at 50 psi (gaugepressure) and then mixed with N2O. What volume of oxygen at 20Cand 50 psi (gauge pressure) should be mixed with 1.7 kg of N2O toget a 50%/50% mixture by volume at 20C? (a) 0.21 m3; (b) 0.27 m3;(c) 1.9 m3; (d) 100 m3
One type of gas mixture used in anesthesiologyis a 50%/50% mixture (by volume) of nitrous oxide (N2O) and oxygen(O2), which can be premixed and kept in a cylinder for later use.Because these two gases don’t react chemically at or below 2000 psi, attypical room temperatures they form a homogeneous single gas phase,which can be considered an ideal gas. If the temperature drops below-6C, however, N2O may begin to condense out of the gas phase. Thenany gas removed from the cylinder will initially be nearly pure O2; asthe cylinder empties, the proportion of O2 will decrease until the gascoming from the cylinder is nearly pure N2O. In another test, the valve of a 500 L cylinder full of the gas mixture at 2000 psi (gauge pressure) is opened wide so that the gas rushes out of the cylinder very rapidly. Why might some N2O condense during this process? (a) This is an isochoric process in which the pressure decreases, so the temperature also decreases. (b) Because of the rapid expansion, heat is…
Aflask_with a v0lume 0f3.16L c0ntains 8g 0f an unkn0wnGas at32oC and 1atm. What is the m0larmass (g/m0l) 0f the gas?
1. The compressibility factor Z = PV/nRT for O2 at -27.1°C and 537.1 atm is 1.50; at 147.4°C and 95.5 atm, it is 1.02. A certain mass of oxygen occupied a volume of 3.28 L at 147.4°C and 95.5 atm. Calculate the volume occupied by the same quantity of oxygen at -27.1°C and 537.1 atm. 2. The composition of a mixture of gases in percentage by volume is 20.5% nitrogen, 15.7% carbon monoxide, 37.8% water, and the rest sulfur dioxide. Calculate the density of the gaseous mixture at 39.8°C and 1.46 atm in grams/liter. Report your answer to the hundredths position.
How much carbon dioxide gas (mole percent) is dissolved in a bottle of sparkling water if the manufacturer used a pressure of 2.68 atm in the bottling process at 25°C? HCO2inwater=1630atm and PsatH2O=3.166kPa at 25°C. Assume xH2O=1.
A gas of pure N2i s confined to a cylinder with a movable piston at one end. The initial pressure of gas is 1.2 x 105 N/m2, the initial volume is 1.0 x 10-3m3, and the initaltemperature is 30oC. (a) How many moles of the gas are in the container? If the piston is compressed so that the pressure is increased to 4.20 x 105 N/m2 and volume is decreased to 5.10 x 10-4m3, what is the new temperature of the gas?
The Ideal Gas Law has more variables than Boyle's Law, and it contains the ideal gas constant, R. The ideal gas law is PV = nRT, where T is the absolute temperature and n is the number of moles of gas present in a system. a. In Boyle's Law, PV = k (a constant). Rearrange the Ideal Gas Law so that the constant R is similarly equal to the variables. b. If PV = k, and PV = nRT as well, express k in terms used in the Ideal Gas Law. c. If you took laboratory syringe setup outside in the summer or put it in the refrigerator, would Boyle's Law be able to adequately describe what would happen to the volume of the system? Why? d. There are other gas laws aside from Boyle's Law, including: Charles' Law (V/T = k), Gay-Lussac's Law (P/T = k), and Avogadro's Law (V/n = k). All these laws feature a "k" value (a constant). What is different about k in these laws compared to the constant R in the Ideal Gas Law?
F 6. A rigid vessel of volume 0.4 m^3 containing H2 at 21.25°C and a pressure of 715x10^3 Pa is connected to a second rigid vessel of volume 0.75m^3 containing Argon at 30.15°C at a pressure of 203x10^3. A valve separating the two vessels is opened and the mixed gases allowed to cool to a temperature of 12.2°C. What is the final pressure of the gas mixture in the connected vessel in atm? (1 atm = 101325 Pa) Please show all steps.
The following system is used for q7-q9 10.00g of O2 and 15.00g N2 are combined in a 20.0L container at 25.00oC O2 32.00g/mol N2 28.02 g/mol R= 0.08206 L atm/mol K What is the mole fraction of the N2 in the system? ( Your answer should have 4 sig figs.)