OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
5th Edition
ISBN: 9781285460369
Author: STANITSKI
Publisher: Cengage Learning
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 8, Problem 101QRT
Interpretation Introduction
Interpretation:
Reason for why measured pressure of acetic acid vapor is comparatively lower than that predicted using
Concept introduction:
Hydrogen bonding: The attractive force that holds two polar molecules (containing Hydrogen and highly electronegative atom, such as N, O, or F) is called as hydrogen boding. This is also called as intermolecular hydrogen bonding.
The hydrogen bonding takes place within a molecule is called as intramolecular hydrogen bonding.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
A student experimentally determines the gas law constant, R, by reacting a small piece of magnesium
with excess hydrochloric acid and then collecting the hydrogen gas over water in a eudiometer. Based
L-atm
on experimentally collected data, the student calculates R to equal 0.0832
mol·K
L-atm
Ideal gas law constant from literature: 0.08206
mol·K
(a) Determine the percent error for the student's R-value.
Percent error =
%
(b) For the statements below, identify the possible source(s) of error for this student's trial.
The student notices a large air bubble in the eudiometer after collecting the hydrogen gas, but
does not dislodge it.
The student does not clean the zinc metal with sand paper.
The student does not equilibrate the water levels within the eudiometer and the beaker at the
end of the reaction. The water level in the eudiometer is 1-inch above the water level in the
beaker.
The student uses the barometric pressure for the lab to calculate R.
A student experimentally determines the gas law constant, R, by reacting a small piece of
magnesium with excess hydrochloric acid and then collecting the hydrogen gas over water
in a eudiometer. Based on experimentally collected data, the student calculates R to equal
L'atm
0.0832
mol·K
L'atm
Ideal gas law constant from literature: 0.08206
mol·K
(a) Determine the percent error for the student's R-value.
Percent error =|1.389
(b) For the statements below, identify the possible source(s) of error for this student's trial.
The student uses the barometric pressure for the lab to calculate R.
The student does not equilibrate the water levels within the eudiometer and the
beaker at the end of the reaction. The water level in the eudiometer is 1-inch
above the water level in the beaker.
The student does not clean the zinc metal with sand paper.
The student notices a large air bubble in the eudiometer after collecting the
hydrogen gas, but does not dislodge it.
A metal cylinder with a capacity of 6.0 L is filled with compressed propane (C3H8). The pressure and temperature of the cylinder when it was initially filled were 120 atm and 75 ◦C, respectively. The molar mass of carbon is 12 g·mol−1 and the molar mass of hydrogen is 1 g·mol−1.
a) How many moles of propane are in the cylinder?
b) What is the mass of the propane inside the cylinder?
c) After some time, the cylinder and its contents cool to 25 ◦C. What is the pressure in the
cylinder after it has cooled?
Chapter 8 Solutions
OWLV2 FOR MOORE/STANITSKI'S CHEMISTRY:
Ch. 8.1 - Prob. 8.1PSPCh. 8.1 - Prob. 8.1ECh. 8.1 - Prob. 8.2ECh. 8.2 - Prob. 8.3CECh. 8.2 - Prob. 8.4CECh. 8.3 - Prob. 8.6CECh. 8.3 - Prob. 8.2PSPCh. 8.3 - Prob. 8.3PSPCh. 8.3 - Prob. 8.4PSPCh. 8.3 - Prob. 8.7CE
Ch. 8.4 - Prob. 8.5PSPCh. 8.4 - Prob. 8.8CECh. 8.4 - Prob. 8.9CECh. 8.4 - Prob. 8.6PSPCh. 8.4 - Prob. 8.10CECh. 8.5 - Prob. 8.7PSPCh. 8.5 - Prob. 8.8PSPCh. 8.5 - Prob. 8.11ECh. 8.6 - Prob. 8.9PSPCh. 8.6 - Prob. 8.12CECh. 8.6 - Prob. 8.13ECh. 8.6 - Prob. 8.10PSPCh. 8.6 - Prob. 8.11PSPCh. 8.7 - Prob. 8.12PSPCh. 8.7 - Prob. 8.14ECh. 8.7 - Prob. 8.16CECh. 8.7 - Prob. 8.17ECh. 8.8 - Prob. 8.13PSPCh. 8.8 - Prob. 8.18ECh. 8.8 - Look up the van der Waals constants, b, for H2,...Ch. 8.11 - List as many natural sources of CO2 as you can,...Ch. 8.11 - Prob. 8.21ECh. 8.11 - Prob. 8.22CECh. 8.11 - Prob. 8.23CECh. 8.11 - Prob. 8.24CECh. 8.12 - Make these conversions for atmospheric...Ch. 8.12 - Prob. 8.25ECh. 8 - In a typical automobile engine, a gasoline...Ch. 8 - Prob. 1QRTCh. 8 - Prob. 2QRTCh. 8 - Prob. 3QRTCh. 8 - Prob. 4QRTCh. 8 - Prob. 5QRTCh. 8 - Prob. 6QRTCh. 8 - Prob. 7QRTCh. 8 - Prob. 8QRTCh. 8 - Prob. 9QRTCh. 8 - Prob. 10QRTCh. 8 - Prob. 11QRTCh. 8 - Prob. 12QRTCh. 8 - Prob. 13QRTCh. 8 - Prob. 14QRTCh. 8 - Prob. 15QRTCh. 8 - Prob. 16QRTCh. 8 - Prob. 17QRTCh. 8 - Prob. 18QRTCh. 8 - Some butane, the fuel used in backyard grills, is...Ch. 8 - Prob. 20QRTCh. 8 - Suppose you have a sample of CO2 in a gas-tight...Ch. 8 - Prob. 22QRTCh. 8 - Prob. 23QRTCh. 8 - Prob. 24QRTCh. 8 - A sample of gas occupies 754 mL at 22 C and a...Ch. 8 - Prob. 26QRTCh. 8 - Prob. 27QRTCh. 8 - Prob. 28QRTCh. 8 - Prob. 29QRTCh. 8 - Prob. 30QRTCh. 8 - Prob. 31QRTCh. 8 - Prob. 32QRTCh. 8 - Calculate the molar mass of a gas that has a...Ch. 8 - Prob. 34QRTCh. 8 - Prob. 35QRTCh. 8 - Prob. 36QRTCh. 8 - Prob. 37QRTCh. 8 - Prob. 38QRTCh. 8 - Prob. 39QRTCh. 8 - Prob. 40QRTCh. 8 - Prob. 41QRTCh. 8 - Prob. 42QRTCh. 8 - Prob. 43QRTCh. 8 - Prob. 44QRTCh. 8 - Prob. 45QRTCh. 8 - Prob. 46QRTCh. 8 - Prob. 47QRTCh. 8 - Prob. 48QRTCh. 8 - The build-up of excess carbon dioxide in the air...Ch. 8 - Prob. 50QRTCh. 8 - Prob. 51QRTCh. 8 - Prob. 52QRTCh. 8 - Prob. 53QRTCh. 8 - Prob. 54QRTCh. 8 - Prob. 55QRTCh. 8 - Benzene has acute health effects. For example, it...Ch. 8 - The mean fraction by mass of water vapor and cloud...Ch. 8 - Acetylene can be made by reacting calcium carbide...Ch. 8 - Prob. 59QRTCh. 8 - You are given two flasks of equal volume. Flask A...Ch. 8 - Prob. 61QRTCh. 8 - Prob. 62QRTCh. 8 - Prob. 63QRTCh. 8 - Prob. 64QRTCh. 8 - Prob. 65QRTCh. 8 - Prob. 66QRTCh. 8 - Prob. 67QRTCh. 8 - Prob. 68QRTCh. 8 - Prob. 69QRTCh. 8 - Prob. 70QRTCh. 8 - Prob. 71QRTCh. 8 - Prob. 72QRTCh. 8 - Prob. 73QRTCh. 8 - Prob. 74QRTCh. 8 - Prob. 75QRTCh. 8 - Prob. 76QRTCh. 8 - Prob. 77QRTCh. 8 - Prob. 78QRTCh. 8 - Prob. 79QRTCh. 8 - Prob. 80QRTCh. 8 - Prob. 81QRTCh. 8 - Prob. 82QRTCh. 8 - Prob. 83QRTCh. 8 - Prob. 84QRTCh. 8 - Prob. 85QRTCh. 8 - Name a favorable effect of the global increase of...Ch. 8 - Prob. 87QRTCh. 8 - Assume that limestone, CaCO3, is used to remove...Ch. 8 - Prob. 89QRTCh. 8 - Prob. 90QRTCh. 8 - Prob. 91QRTCh. 8 - Prob. 92QRTCh. 8 - Prob. 93QRTCh. 8 - Prob. 94QRTCh. 8 - Prob. 95QRTCh. 8 - Prob. 96QRTCh. 8 - Prob. 97QRTCh. 8 - Prob. 98QRTCh. 8 - Prob. 99QRTCh. 8 - Prob. 100QRTCh. 8 - Prob. 101QRTCh. 8 - Prob. 102QRTCh. 8 - Prob. 103QRTCh. 8 - Prob. 104QRTCh. 8 - Prob. 105QRTCh. 8 - Prob. 106QRTCh. 8 - Prob. 107QRTCh. 8 - Prob. 108QRTCh. 8 - Prob. 109QRTCh. 8 - Consider these four gas samples, all at the same...Ch. 8 - Prob. 111QRTCh. 8 - Prob. 112QRTCh. 8 - Prob. 113QRTCh. 8 - Prob. 114QRTCh. 8 - Prob. 115QRTCh. 8 - Prob. 116QRTCh. 8 - Prob. 117QRTCh. 8 - Prob. 118QRTCh. 8 - Prob. 119QRTCh. 8 - Prob. 120QRTCh. 8 - Prob. 121QRTCh. 8 - Prob. 122QRTCh. 8 - Prob. 123QRTCh. 8 - Prob. 124QRTCh. 8 - Prob. 125QRTCh. 8 - Prob. 126QRTCh. 8 - Prob. 127QRTCh. 8 - Prob. 128QRTCh. 8 - Prob. 129QRTCh. 8 - Prob. 8.ACPCh. 8 - Prob. 8.BCP
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Similar questions
- Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?arrow_forwardWhat possible uses exist for the natural gas liquids that are removed from natural gas during its processing?arrow_forwardDetermine the total pressure in the flask when 1.02 atm of Oz is added to a 1.95 L flask containing 145 mL ethanol (CH3CH2OH). The density of ethanol is 703.00 kg/m. The temperature remains at 100 °C throughout the reaction. Note that the total pressure is calculated by adding up the pressure of ALL gases (O2, CO2, and H2O in this case).arrow_forward
- The ideal gas law describes the relationship between pressure (P), temperature (T), volume (V), and the number of moles of gas (n). PV = nRT The additional symbol, R, represents the ideal gas constant. The ideal gas law is a good approximation of the behavior of gases when the pressure is low and the temperature is high. (What constitutes low pressure and high temperature varies with different gases.) In 1873, Johannes Diderik van der Waals proposed a modified version of the ideal gas law that better models the behavior of real gases over a wider range of temperature and pressure. na P + ")(v – nb) = nRT In this equation the additional variables a and b represent values characteristic of individual gases.arrow_forward5. An experiment is performed to measure the mass percent of CaCO3(s) in eggshells. Five different samples of CaCO3(s) of known mass react with an excess of 2.0M HCl(aq) in identical sealed, rigid reaction vessels. The pressure of the gas produced is measured with a pressure gauge attached to the reaction vessel. Since the reaction is exothermic, the reaction system is cooled to its original temperature before Cooling the HCl(aq) to a lower temperature than it was in the original experiment the pressure is recorded. The experimental data are used to create the calibration line below. Using eggshells that are more finely powdered than those used in the original experiment 0.10- 0.09 0.08- Using 2.0M CH3COOH(aq) instead of 2.0M HCl(aq) 0.07 * 0.06- Reducing the volume of the reaction vessel 0.05 0.04 CLEAR ALL 0.03- 0.02- 0.05 0.10 0.15 0.20 Mass of CaCO3(s) (grams) The experiment is repeated with an eggshell sample, and the experimental data are recorded in the table below. Mass of…arrow_forwardAt 1.00 atm and 0 °C, a 5.04 L mixture of methane (CH4) and propane (C₂H) was burned, producing 18.7 g CO₂. What was the mole fraction of each gas in the mixture? Assume complete combustion. Xmethane = Xpropane =arrow_forward
- Please write to their unit.arrow_forwardJj.200.arrow_forwardConsider the reaction: 2 NO(g) + Br2(g) =2 NOBr(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br2) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBR at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L·bar/mol· K and MW of Br2 is 159.808 g/mol.) Calculate the Kp. Incorrect, 1 attempt remaining Your submission: Feedback: Use PV=nRT to determine the initial pressures of the reactants. You can then determine the pressures of the reactants equilibrium by subtracting the pressure that reacted. Kp = P(NOBr)*/P(NO)²*P(Br)2 43.8 %3Darrow_forward
- Calculate the total pressure (in atm) of a mixture of 3.00 x 10-2 mol of helium, He, and 7.00 x 10- mol of oxygen, O2, in a 6.00 L flask at 20.°C. Assume ideal gas behavior. Total pressure atm ||arrow_forwardA 5.50-mole sample of NH3 gas is kept in a 1.85-L container at 309 K. If the van der Waals equation is assumed to give the correct answer for the pressure of the gas, calculate the percent error made in using the ideal-gas equation to calculate the pressure. (Use a = 4.17 atm·L2·mol−2 and b = 0.0371 L·mol−1 for the van der Waals equation.)arrow_forwardConsider the reaction: 2 NO(g) + Br2(g) =2 NOBI(g) A chemist placed 0.0322 mol of NO and 1.70 g of bromine (Br2) into a sealed 1.00 L reaction vessel and then allowed the reaction to reach equilibrium. The pressure of the NOBR at equilibrium at 25.0°C is 0.444 bar. (R = 0.08314 L·bar/mol·K and MW of Br2 is 159.808 g/mol.) Calculate the Kp.arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
General Chemistry - Standalone book (MindTap Cour...ChemistryISBN:9781305580343Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; DarrellPublisher:Cengage Learning
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
Introduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry: Matter and Change
Chemistry
ISBN:9780078746376
Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl Wistrom
Publisher:Glencoe/McGraw-Hill School Pub Co
General Chemistry - Standalone book (MindTap Cour...
Chemistry
ISBN:9781305580343
Author:Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Cengage Learning
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Introduction to General, Organic and Biochemistry
Chemistry
ISBN:9781285869759
Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar Torres
Publisher:Cengage Learning