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Concept explainers
(a)
Interpretation:
The pressure should be calculated on the basis of given information at constant temperature.
Concept Introduction:
According to Boyle’s law pressure is inversely proportional to the volume of gas at constant temperature and amount of gas.
It expresses as; P1 V1 = P2 V2.
(b)
Interpretation:
The volume should be calculated on the basis of given information at constant temperature.
Concept Introduction:
According to Boyle’s law pressure is inversely proportional to the volume of gas at constant temperature and amount of gas.
It expresses as; P1 V1 = P2 V2.
(c)
Interpretation:
The volume should be calculated on the basis of given information at constant temperature.
Concept Introduction:
According to Boyle’s law pressure is inversely proportional to the volume of gas at constant temperature and amount of gas.
It expresses as; P1 V1 = P2 V2.
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Chapter 13 Solutions
Introductory Chemistry: A Foundation
- 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?arrow_forwardIn an experiment in a general chemistry laboratory, a student collected a sample of a gas over water. The volume of the gas was 265 mL at a pressure of 753 torr and a temperature of 27 C. The mass of the gas was 0.472 g. What was the molar mass of the gas?arrow_forwardMake the indicated pressure conversions. msp;a.1.54105Patoatmospheresb.1.21atmtopascalsc.97,345PatommHgd.1.32kPatopascalsarrow_forward
- A 1 007-g sample of an unknown gas exerts a pressure of 715 mm Hg in a 452-mL container at 23 C. What is the molai mass of the gas?arrow_forward2. The volume of a gas sample is 235 mL at a temperature of 25 ℃. At what temperature would that same gas sample have a volume of 310. mL, if the pressure of the gas sample is held constant? −47.0 ℃ 69.4 ℃ 33.1 ℃ 120.℃arrow_forward93 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.)arrow_forward
- 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?arrow_forward5-118 Isooctane, which has a chemical formula C8H18 is the component of gasoline from which the term octane rating derives. (a) Write the balanced chemical equation for the combustion of isooctane. (b) The density of isooctane is 0.792 g/mL. How many kg of C02 are produced each year by the annual U.S. gasoline consumption of L? (c) What is the volume in liters of this CO2 at STP? (d) The chemical formula for isooctane can be represented by (CH3)3CCH2CH(CH3)2. Draw a Lewis structure of isooctane. (e) Another molecule with the same molecular formula is octane, which can be represented by: When comparing isooctane and octane, one structure is observed to have a boiling point of 99°C, while another is known to have a boiling point Of 125°C. Which substance, isooctane or octane, is expected to have the higher boiling point? (f) Determine whether isooctane or octane is expected to have the greater vapor pressure.arrow_forwardA cylinder of a gas mixture used for calibration of blood gas analyzers in medical laboratories contains 5.0% CO2, 12.0% O2, and the remainder N2 at a total pressure of 146 atm. What is the partial pressure of each component of this gas? (The percentages given indicate the percent of the total pressure that is due to each component.)arrow_forward
- A 1.000-g sample of an unknown gas at 0C gives the following data: P(atm) V (L) 0.2500 3.1908 0.5000 1.5928 0.7500 1.0601 1.0000 0.7930 Use these data to calculate the value of the molar mass at each of the given pressures from the ideal gas law (we will call this the apparent molar mass at this pressure). Plot the apparent molar masses against pressure and extrapolate to find the molar mass at zero pressure. Because the ideal gas law is most accurate at low pressures, this extrapolation will give an accurate value for the molar mass. What is the accurate molar mass?arrow_forward61 As one step in its purification, nickel metal reacts with carbon monoxide to form a compound called nickel tetracarbonyl, Ni(CO)4, which is a gas at temperature above about 316 K. A 2.000-L flask is filled with CO gas to a pressure of 748 torr at 350.0 K, and then 5.00 g of Ni is added. If the reaction describe occurs and goes to completion at constant temperature, what will the final pressure in the falsk be?arrow_forwardWhich of the following statements is(are) true? a. If the number of moles of a gas is doubled, the volume will double, assuming the pressure and temperature of the gas remain constant. b. If the temperature of a gas increases from 25C to 50C, the volume of the gas would double, assuming that the pressure and the number of moles of gas remain constant. c. The device that measures atmospheric pressure is called a barometer. d. If the volume of a gas decreases by one half, then the pressure would double, assuming that the number of moles and the temperature of the gas remain constant.arrow_forward
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningGeneral, Organic, and Biological ChemistryChemistryISBN:9781285853918Author:H. Stephen StokerPublisher:Cengage LearningChemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
- Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage LearningPhysical ChemistryChemistryISBN:9781133958437Author:Ball, David W. (david Warren), BAER, TomasPublisher:Wadsworth Cengage Learning,Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
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