1,2,3,4 100%Normal textFjalla One1. A canister containing air has a volume of 85 cm' and a pressure of 1.45 atm when the temper:What is the pressure when the volume is increased to 180 cm and the temperature is reduced2. Air is transferred from a 75 L tank where the pressure is 125 psi and the temperature is 288 Kvolume of 6.1 L and a pressure of 25 psi. What is the new temperature?3. A helium balloon at 28°C has a volume of 1.8 L and a pressure of 102 kPa. What is the volumballoon when is rises into the atmosphere where the pressure is 85 kPa and the temperature is4. The pressure of a piston with a volume of 650 cm' and 85°C is 30 torr. It is heated to 350°Ccompressed to a volume of 65 cm', What is the new pressure?5. A gas tank has a volume of 28 1 m' and a pressure of 18.4 atm. The temperature of the gas ithe Celsius temperature when the gas is put in an 11.2 m' tank with a pressure of 22.7 at 26. A metal can is able to withstand 3800 kPa before is bursts. The gas in the can has a volume ofthepressureis 110 kPa at 25°C. If the can is crushed to a volume of 8.5 mL and the tem2.

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Chemistry

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Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section: Chapter Questions

Problem 114AP

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Helium gas, He, at 22C and 1.00 atm occupied a vessel whose volume was 2.54 L. What volume would this gas occupy if it were cooled to liquid-nitrogen temperature (197C)?
Pressures of gases in mixtures are referred to as partial pressures and are additive. 1.00 L of He gas at 0.75 atm is mixed with 2.00 L of Ne gas at 1.5 atm at a temperature of 25.0 C to make a total volume of 3.00 L of a mixture. Assuming no temperature change and that He and Ne can be approximated as ideal gases, what are a the total resulting pressure, b the partial pressures of each component, and c the mole fractions of each gas in the mix?
93 The complete combustion of octane can be used as a model for the burning of gasoline: 2C8H18+25O216CO2+18H2O Assuming that this equation provides a reasonable model of the actual combustion process, what volume of air at 1.0 atm and 25°C must be taken into an engine to burn 1 gallon of gasoline? (The partial pressure of oxygen in air is 0.21 atm and the density of liquid octane is 0.70 g/mL.)
Under what conditions does the behavior of a real gas begin to differ significantly from the ideal gas law?
A tank is filled with gas to a pressure of 875 mm Hg at 25C. The gas is transferred without loss to a tank twice the size of the original tank. If the pressure is to remain constant, at what temperature (in C) should the tank be kept?
What is the temperature of an 11.2-L sample of carbon monoxide, CO, at 744 torr if it occupies 13.3 L at 55 C and 74-4 torr?
Referring to exercises 1.6 and 1.7, does it matter if the pressure difference is caused by an ideal gas or a non-ideal gas? Explain your answer.
97 Homes in rural areas where natural gas service is not available often rely on propane to fuel kitchen ranges. The propane is stored as a liquid, and the gas to be burned is produced as the liquid evaporates. Suppose an architect has hired you to consult on the choice of a propane tank for such a new home. The propane gas consumed in 1.0 hour by a typical range burner at high power would occupy roughly 165 L at 25°C and 1.0 atm, and the range chosen by the client will have six burners. If the tank under consideration holds 500.0 gallons of liquid propane, what is the minimum number of hours it would take for the range to consume an entire tankful of propane? The density of liquid propane is 0.5077 kg/L.
A certain flexible weather balloon contains helium gas at a volume of 855 L. Initially, the balloon is at sea level where the temperature is 25C and the barometric pressure is 730 torr. The balloon then rises to an altitude of 6000 ft, where the pressure is 605 torr and the temperature is 15C. What is the change in volume of the balloon as it ascends from sea level to 6000 ft?
Urea (H2NCONH2) is used extensively as a nitrogen source in fertilizers. It is produced commercially from the reaction of ammonia and carbon dioxide: 2NH3(g)+CO2(g)PressureHeatH2NCONH2(s)+H2O(g) Ammonia gas at 223C and 90. atm flows into a reactor at a rate of 500. L/min. Carbon dioxide at 223C and 45 atm flows into the reactor at a rate of 600. L/min. What mass of urea is produced per minute by this reaction assuming 100% yield?
A four-liter tank is filled with propane gas, C3H8. The mass of the tank filled with gas is 1236 g. The pressure in the tank is 2.68 atm. The temperature in the room is 37C. The propane in the tank is used up under the same conditions of temperature and pressure. What is the mass of the empty tank?
Explain why the plot of PV for CO2 differs from that of an ideal gas.

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