Review I Constants Periodic TableFor every 10 m below the water surface, thepressure exerted by the water adds 14.7 psi toatmospheric pressure, so 10 m below the surfacewould have a total pressure of 29.4 psi.Part AYou maywant to reference (Pages 272 - 279)Section 7.2 while completing this problem.If a swimmer has a lung volume of 6 L at sea level, what would the volume of her lungsbe when she is at the bottom of a pool that is 5.0 m deep? Assume that thetemperature and amount of the air in the lungs remain unchanged.Express your answer to two significant figures and include the appropriate units.7НА?ValueUnitsSubmitRequest AnswerP Pearson2019 Pearson Education Inc. All rights reserved. | Terms of Use Privacy Policy Permissions | Contact UsCopyrightTALL DOtrvey ToTTITCTIOETSOnly 2 left in stock - order soon.Only 10 left in stock - order30,639ОСТ28g0F3FIFIOF9F8F5F6F7F4*HARDO

Given,Pressure of the lungs at sea level (P1) = atmospheric pressure = 1 atm = 14.7 psiVolume of the…

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Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter5: Gases

Section: Chapter Questions

Problem 5.60PAE: 60 Automakers are always investigating reactions for the generation of gas to inflate air bags, in...

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If the gas inside the flask in the above exercise is cooled sothat its pressure is reduced to a value of 715.7 torr, what will be the height of the mercury in the open-ended arm?(Hint: The sum of the heights in both arms must remainconstant regardless of the change in pressure.)(a) 49.0 mm (b) 95.6 mm (c) 144.6 mm (d) 120.1 mm
If the gas inside the flask in the above exercise is cooled sothat its pressure is reduced to a value of 715.7 torr, what willbe the height of the mercury in the open-ended arm?(Hint: The sum of the heights in both arms must remainconstant regardless of the change in pressure.)(a) 49.0 mm (b) 95.6 mm (c) 144.6 mm (d) 120.1 mm
Use the van der Waals equation to calculate the pressure (atm) exerted by 1.57 mol Cl_{2}2(g) confined to a volume of 1.50 L at 273K. For Cl_{2}2, a = 6.49 L^{2}2atm mol^{-2}−2, b = 0.0562 L mol^{-1}−1.
25 L of a gas were collected over water when the barometer read 505.0 mmHg and the temperature was 48 oC . What volume would the dry gas occupy at standard conditions? HINT: Consider Dalton’s law of partial pressures.
A sample of a smoke stack emission was collected into a 1.35-L tank at742 mm Hg and analyzed. The analysis showed 92% CO2, 2.6% NO,1.2 % SO2, and 4.1% H2O by mass. What is the partial pressure exerted by eachgas?
Use Gay-Lussac equation to solve the given problem."1. A certain light bulb containing argon has a pressure 1.20 atm at 18 0 C. If it will be heated to 850C atconstant volume, what will be the resulting pressure ( P2 )? Is it enough to cause sudden breakage of thebulb?2. At 293 K a confined ammonia gas has a pressure of 2.50 atm. At what temperature ( T2 ) would itspressure be equal to 760 mmHg ?
A 200-cm3 vessel contains hydrogen gas at a temperatureof 25°C and a pressure of 0.990 atm. Unfortunately, thevessel has a tiny hole in its wall, and over a period of1 hour, the pressure drops to 0.989 atm. What is theradius of the hole (assumed to be circular)?
41 A sample of a smokestack emission was collected into 1.25-L tank at Hg and analyzed. The analysis showed 92% CO2, 3.6% NO, 1.2% SO2, and 4.1% H2O by mass. What is the partial pressure exerted by gas?
What is the density of laughing gas, dinitrogen monoxide, N2O, at a temperature of 325 K and a pressure of 113.0 kPa?
60 Automakers are always investigating reactions for the generation of gas to inflate air bags, in part the because the sodium produced in the decomposition of NaN3 (see Problem 5.59) presents safety concerns. One system that has been considering is the oxidation of graphite by Strontium nitrate, as Sr(NO3)2as shown in the equation below: 5C(s)+2Sr(NO3)2(s)2SrO(s)+2N2(g)+5CO2(g) . Suppose that a System is being designed using this reaction and the goal is to generate enough gas to inflate a bag 61 L and 1.3 atm at 23 C. What is the minimum mass of graphite that should be used in the design of this system?
Metallic molybdenum can be produced from the mineral molybdenite, MoS2. The mineral is first oxidized in air to molybdenum trioxide and sulfur dioxide. Molybdenum trioxide is then reduced to metallic molybdenum using hydrogen gas. The balanced equations are MoS2(s)+72O2(g)MoO3(s)+2SO2(g)MoO3(s)+3H2(g)Mo(s)+3H2O(l) Calculate the volumes of air and hydrogen gas at 17C and 1.00 atm that are necessary to produce 1.00 103 kg pure molybdenum from MoS2. Assume air contains 21% oxygen by volume, and assume 100% yield for each reaction.
A weather balloon contains 8.80 moles of helium at a pressure of 0.992 atm and a temperature of 25 C at ground level. What is the volume of the balloon under these conditions?

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