Calculating pressure-volume work BryAnna 1/5 A mixture of krypton and argon gas is expanded from a volume of 37.0 L to a volume of 47.0 L, while the pressure is held constant at 83.0 atm. Calculate the work done on the gas mixture: Round your answer to 3 significant digits, and be sure it has the correct sign (positive or negative). Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibilit image_50376449.JPG image_50371073.JPG D image_50353665.JPG 2 ECHE.docx MacBook Air F7 F8

Calculating pressure-volume work BryAnna 1/5 A mixture of krypton and argon gas is expanded from a volume of 37.0 L to a volume of 47.0 L, while the pressure is held constant at 83.0 atm. Calculate the work done on the gas mixture: Round your answer to 3 significant digits, and be sure it has the correct sign (positive or negative). Explanation Check © 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center Accessibilit image_50376449.JPG image_50371073.JPG D image_50353665.JPG 2 ECHE.docx MacBook Air F7 F8

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 37E: Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40....

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In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
Ethyl alcohol, C2H5OH, is the intoxicating agent in liquor. Burning 1.00 g of ethyl alcohol in an excess of oxygen at 23.28C and constant volume releases 29.52 kJ of heat. When 7.40 g of ethyl alcohol is burned in oxygen under the same conditions in a bomb calorimeter, the temperature of the bomb and water rises from 23.28C to 48.04C. The bomb holds 0.750 kg of water. (a) What is q for the combustion of the ethyl alcohol in the bomb calorimeter? (b) What is qH2O? (c) What is qcal? (d) What is the heat capacity of the calorimeter?
What will be the final temperature of a mixture made from equal masses of the following: water at 25.0C, ethanol at 35.5C, and iron at 95C?
Calculate the heat capacity, in joules and in calories per degree, of the following: (a) 45.8 g of nitrogen gas (b) 1.00 pound of aluminum metal
Suppose that you are studying kinetic energy of helium molecules: A helium weather balloon rises to an altitude of 40,000 ft; the temperature of the gas drops to 70 F. (a) Make an appropriate choice of system and surroundings and describe it unambiguously. (b) Explain why you chose the system and surroundings you did. (c) Identify transfers of energy and material into and out of the system that would be important for you to monitor in your study.
A beaker of water at 400 C(on the left in the drawing) and a beaker of ice water at 0 C are placed side by side in an insulated container. After some time has passed, the temperature of the water in the beaker on the left is 30 C and the temperature of the ice water is still 0 C. Describe what is happening in each beaker (a) on the molecular level and (b) in terms of the second law of thermodynamics.
On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm (STP) evolves 75.65 kJ of heat. If the gas is a mixture of ethane (C2H6) and propane (C3H8), what is the mole fraction of ethane in the mixture?
Acetic acid, HC2H3O2, is responsible for the sour taste of vinegar. Combustion of acetic acid gives off 14.52 kJ/g of heat. When 15.00 g of acetic acid is burned in a bomb calorimeter (heatcapacity=2.166kJ/C) containing 0.800 kg of water, the final temperature in the calorimeter is 64.14C. What was the initial temperature of the calorimeter?
Consider a mixture of air and gasoline vapor in a cylinder with a piston. The original volume is 40. cm3. If the combustion of this mixture releases 950. J of energy, to what volume will the gases expand against a constant pressure of 650. torr if all the energy of combustion is converted into work to push back the piston?
Calculate the heat capacity, in joules and in calories per degree, of the following: (a) 28.4 g of water (b) 1.00 oz of lead
Nitrogen gas is confined in a cylinder with a movable piston under a constant pressure of 9.95 104 Pa. When 695 J of energy in the form of heat is transferred from the gas to the surroundings, its volume decreases by 1.88 L. What is the change in internal energy of the gas?
During a recent winter month in Sheboygan, Wisconsin, it was necessary to obtain 3500 kWh of heat provided by a natural gas furnace with 89% efficiency to keep a small house warm (the efficiency of a gas furnace is the percent of the heat produced by combustion that is transferred into the house). (a) Assume that natural gas is pure methane and determine the volume of natural gas in cubic feet that was required to heat the house. The average temperature of the natural gas was 56 F; at this temperature and a pressure of 1 atm, natural gas has a density of 0.68 1 g/L. (b) How many gallons of LPG (liquefied petroleum gas) would be required to replace the natural gas used? Assume the LPG is liquid propane [ C3H8 : density, 0.5318 g/mL; enthalpy of combustion, 2219 Id/mo for the formation of CO2(g) and H2O(l) ] and the furnace used to burn the LPG has the same efficiency as the gas furnace. (c) What mass of carbon dioxide is produced by combustion of the methane used to heat the house? (d) What mass of water is produced by combustion of the methane used to heat the house? (e) What volume of air is required to provide the oxygen for the combustion of the methane used to heat the house? Air contains 23% oxygen by mass. The average density of air during the month was 1.22 g/L. (f) How many kilowatt—hours ( 1kWh=3.6106 J) of electricity would be required to provide the heat necessary to heat the house? Note electricity is 100% efficient in producing heat inside a house. (g) Although electricity is 100% efficient in producing heat inside a house, production and distribution of electricity is not 100% efficient. The efficiency of production and distribution of electricity produced in a coal-fired power plant is about 40%. A certain type of coal provides 2.26 kWh per pound upon combustion. What mass of this coal in kilograms will be required to produce the electrical energy necessary to heat the house if the efficiency of generation and distribution is 40%?