Chemistry: The Molecular Nature of Matter
7th Edition
ISBN: 9781118516461
Author: Neil D. Jespersen, Alison Hyslop
Publisher: WILEY
expand_more
expand_more
format_list_bulleted
Concept explainers
Question
Chapter 10, Problem 61RQ
Interpretation Introduction
Interpretation:
The volume of carbon dioxide in milliliters at a given temperature and pressure that could be formed in the combustion of carbon monoxide is to be calculated.
Concept Introduction:
The effect of temperature and pressure on the volume of a gas is given by an equation called the ideal gas equation. It is expressed as follows:
Here, is the pressure, is the volume, is the number of moles, is the gas constant, and is the temperature.
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solutionStudents have asked these similar questions
Determine 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).
Sulfur dioxide reacts with oxygen in the presence of plati-
num to give sulfur trioxide:
2 SO2(g) + O2(g) → 2 SO3(g)
Suppose that at one stage in the reaction, 26.0 mol SO2,
83.0 mol O2, and 17.0 mol SO3 are present in the reaction
vessel at a total pressure of 0.950 atm. Calculate the mole
fraction of SO3 and its partial pressure.
The volume of a sample of pure HCl gas was 4.102 L at 25 oC and 102 torr. It was completely dissolved in an aqueous solution. Then this solution of HCl(aq) was titrated to the end point with 15 mL of NaOH(aq). What was the molar concentration of NaOH(aq)?
Chapter 10 Solutions
Chemistry: The Molecular Nature of Matter
Ch. 10 - Prob. 1PECh. 10 - Prob. 2PECh. 10 - Prob. 3PECh. 10 - Prob. 4PECh. 10 - Prob. 5PECh. 10 - Prob. 6PECh. 10 - Prob. 7PECh. 10 - Prob. 8PECh. 10 - Prob. 9PECh. 10 - Prob. 10PE
Ch. 10 - Practice Exercise 10.11 How many grams of argon...Ch. 10 - Prob. 12PECh. 10 - Practice Exercise 10.13
The label on a cylinder of...Ch. 10 - A glass bulb is found to have a volume of 544.23...Ch. 10 - Sulfur dioxide is a gas that has been used in...Ch. 10 - Radon, a radioactive gas, is formed in one step of...Ch. 10 - Practice Exercise 10.17
A gaseous compound of...Ch. 10 - A compound composed of only carbon and hydrogen...Ch. 10 - Carbon disulfide is an extremely flammable liquid....Ch. 10 - In one lab, thegas-collecting apparatus used a gas...Ch. 10 - The explosive PETN, pentaerythritoltetranitrate,...Ch. 10 - Prob. 22PECh. 10 - Suppose you prepared a sample of nitrogen and...Ch. 10 - A 2.50 L sample of methane was collected over...Ch. 10 - Suppose a mixture containing 2.15 g H2 and 34.0 g...Ch. 10 - Sulfur dioxide and oxygen react according to the...Ch. 10 - Bromine has two isotopes with masses of 78.9 and...Ch. 10 - The hydrogen halide gases all have the same...Ch. 10 - Prob. 1RQCh. 10 - Prob. 2RQCh. 10 - Prob. 3RQCh. 10 - Prob. 4RQCh. 10 - Prob. 5RQCh. 10 - Prob. 6RQCh. 10 - Prob. 7RQCh. 10 - What is meant by an ideal gas? Under what...Ch. 10 - Prob. 9RQCh. 10 - Prob. 10RQCh. 10 - Prob. 11RQCh. 10 - Prob. 12RQCh. 10 - Prob. 13RQCh. 10 - Prob. 14RQCh. 10 - Prob. 15RQCh. 10 - Prob. 16RQCh. 10 - Prob. 17RQCh. 10 - Prob. 18RQCh. 10 - Prob. 19RQCh. 10 - Prob. 20RQCh. 10 - Prob. 21RQCh. 10 - Prob. 22RQCh. 10 - Prob. 23RQCh. 10 - Prob. 24RQCh. 10 - Prob. 25RQCh. 10 - Prob. 26RQCh. 10 - Prob. 27RQCh. 10 - Prob. 28RQCh. 10 - Prob. 29RQCh. 10 - Prob. 30RQCh. 10 - What does a small value for the van der Waals...Ch. 10 - Which of the molecules below has the larger value...Ch. 10 - Under the same conditions of T and V, why is the...Ch. 10 - Prob. 34RQCh. 10 - Carry out the following unit conversions: (a) 1.26...Ch. 10 - Prob. 36RQCh. 10 - Prob. 37RQCh. 10 - 10.38 What is the pressure in atm of each of the...Ch. 10 - 10.39 An open-end manometer containing mercury was...Ch. 10 - Prob. 40RQCh. 10 - Prob. 41RQCh. 10 - An open-end mercury manometer was connected to a...Ch. 10 - Prob. 43RQCh. 10 - 10.44 Suppose a gas is in a vessel connected to...Ch. 10 - Prob. 45RQCh. 10 - Prob. 46RQCh. 10 - Prob. 47RQCh. 10 - Prob. 48RQCh. 10 - Prob. 49RQCh. 10 - Prob. 50RQCh. 10 - A sample of helium at a pressure of 74$ torr and...Ch. 10 - When a sample of neon with a volume of 648 mL and...Ch. 10 - What must be the new volume of a sample of...Ch. 10 - When 286 mL of oxygen at 741 torr and 18.0C was...Ch. 10 - A sample of argon with a volume of 6.18 L, a...Ch. 10 - Prob. 56RQCh. 10 - How many milliliters of O2 are consumed in the...Ch. 10 - How many milliliters of oxygen are required to...Ch. 10 - *10.59 How many milliliters of measured at and...Ch. 10 - How many milliliters of H2O vapor, measured at...Ch. 10 - Prob. 61RQCh. 10 - Prob. 62RQCh. 10 - Prob. 63RQCh. 10 - Prob. 64RQCh. 10 - Prob. 65RQCh. 10 - Prob. 66RQCh. 10 - Prob. 67RQCh. 10 - Prob. 68RQCh. 10 - Prob. 69RQCh. 10 - 10.70 Methane is formed in landfills by the action...Ch. 10 - A chemist isolated a gas in a glass bulb with a...Ch. 10 - Prob. 72RQCh. 10 - 10.73 To three significant figures, calculate the...Ch. 10 - To three significant figures, calculate the...Ch. 10 - 10.75 What density does oxygen have at and 742...Ch. 10 - At 748.0 torr and 20.65C, what is the density of...Ch. 10 - The explosive PETN, pentaerythritol tetranitrate,...Ch. 10 - TNT, trinitrotoluene, is an explosive that can...Ch. 10 - Propylene, C3H6, reacts with hydrogen under...Ch. 10 - Nitric acid is formed when NO2 is dissolved in...Ch. 10 - A mixture of gases contains 315 torr N2, 275 torr...Ch. 10 - Prob. 82RQCh. 10 - A 1.00 L container was filled by pumping into it...Ch. 10 - A special gas mixture, BAR 97 High without NO, is...Ch. 10 - Prob. 85RQCh. 10 - Prob. 86RQCh. 10 - A 22.4 L container at 0C contains 0.300 mol N2,...Ch. 10 - A mixture of N2,O2,andCO2 Has a total pressure of...Ch. 10 - A 0.200 mol sample of a mixture of N2 and CO2 with...Ch. 10 - A sample of carbon monoxide was prepared and...Ch. 10 - Prob. 91RQCh. 10 - What volume of wet oxygen would you have to...Ch. 10 - Prob. 93RQCh. 10 - Prob. 94RQCh. 10 - Prob. 95RQCh. 10 - 10.96 For the gases which gas will effuse the...Ch. 10 - Prob. 97RQCh. 10 - Prob. 98RQCh. 10 - Uranium hexafluoride is a white solid that readily...Ch. 10 - Prob. 100RQCh. 10 - Prob. 101RQCh. 10 - A typical automobile has a weight of approximately...Ch. 10 - *10.103 Suppose you were planning to move a house...Ch. 10 - Prob. 104RQCh. 10 - Two flasks (which we will refer to as flask 1 and...Ch. 10 - *10.106 A bubble of air escaping from a divers...Ch. 10 - *10.107 In a diesel engine, the fuel is ignited...Ch. 10 - *10.108 Early one cool (60.0F) morning you start...Ch. 10 - Prob. 109RQCh. 10 - *10.110 A mixture was prepared in a 0.500 L...Ch. 10 - *10.111 A student collected 18.45 mL of H2 over...Ch. 10 - *10.112 A mixture of gases is prepared from 87.5 g...Ch. 10 - 10.113 A gas was found to have a density of...Ch. 10 - *10.114 In one analytical procedure for...Ch. 10 - Prob. 115RQCh. 10 - Prob. 116RQCh. 10 - Prob. 117RQCh. 10 - The odor of a rotten egg is caused by hydrogen...Ch. 10 - Chlorine reacts with sulfite ion to give sulfate...Ch. 10 - *10.120 In an experiment designed to prepare a...Ch. 10 - Carbon dioxide can be made in the lab by the...Ch. 10 - 10.122 Boron forms a variety of unusual compounds...Ch. 10 - Prob. 123RQCh. 10 - Carbon dioxide is implicated in global warming....Ch. 10 - Prob. 125RQCh. 10 - One of the that is implicated in decreasing the...
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
- How does hydraulic fracturing differ from previously used techniques for the recovery of natural gas from the earth?arrow_forwardCalculate the number of CO molecules in 1.1 L of this air at a pressure of 760 torr and a temperature of 22 ∘C.arrow_forwardWhat volume of carbon dioxide gas (in mL) at 834 mm Hg and 25 °C can be produced when 2.3 g of MgCO3(s) are put into an Erlenmeyer flask containing 289 mL of 0.171 M HCl(aq) ?1 MgCO3(s) + 2 HCl(aq) → MgCl2(aq) + CO2(g) + H2O(l)arrow_forward
- What volume of gas (ml) can be produced the complete reaction of 3.82 g of calcium sulfite with excess HCL (aq), when the final pressure of the gas in the reaction vessel is 827 torr at 44°C.arrow_forwardQ1 (a) 3.2 g of sulphur was produced in a reaction between 6.0 L of hydrogen sulfide gas with excess an amount of sulphur dioxide. With the aid of Table Q1 (a)(i) and Table Q1 (a)(ii), predict the temperature (in °C) of the reaction if it was conducted at 750 torr. Element Actinium Aluminum Americium Antimony Argon Arsenic Astatine Barium Berkelium Beryllium Bismuth Boron Bromine Cadmium Calcium Californium Carbon Cerium Cesium Chlorine Chromium Cobalt Copper Curiam CY с Ce Cs a Cr Co Ca Cm Dysprosium Dy Einsteinium Es Er Eu Fm F Fr Gd Ga Ge Erbium Europium Fermium Fluorine Francium Gadoliniam Gallium Germaniam Gold Hafnium Helium Holmium Hydrogen Indium Iodine Iridium Iron Krypton Lanthanam Lawrencium Lead Lithiam Lutetium Table Q1 (a)(i): Atomic Number and Atomic Mass of Elements Magnesium Manganese Symbol Ac Al Am Sb As Al Ba Bk Be Bi B Br Ca Hr He Ho H In I Ir Fe Kr La Lr Ph Li Lu Mg Mn Atomic number (2) 89 13 95 51 18 33 85 56 97 4 83 5 35 48 20 98 6 58 55 17 24 27 29 96 66 99 68…arrow_forwardThe temperature of your water was 22.4 degrees Celsius. The volume of hydrogen collected was 35.3 mL. The atmospheric pressure in the lab room was 29.60 inches Hg. The difference in the water level between the beaker and the burette is 20.0 cm. What was the mass of the magnesium ribbon used? Hint: 2 HCl(aq) + Mg(aq) = H2(g) + MgCl2(aq)arrow_forward
- Please answer questions 1-3 Please refer to the picture below:arrow_forwardGiven the following reaction of Ca(s) in HCl(aq): Ca(s) + 2 HCl(aq) --> CaCl2(aq) + H2(g) If 32.7g of calcium solid are placed in this reaction and at the end of the experiment, hydrogen gas is produced at 25.000C and with a pressure of 790. mmHg. Calculate the volume of hydrogen gas produced.arrow_forwardOn a day with a temperature of 15 ∘C and a pressure of 780.0 torr , how many grams of peroxyacyl nitrates are found in the air above Los Angeles (1500 km3) if the concentration is 30.0 mol of peroxyacetyl nitrate per 1 billion moles of air (30 ppb)? The molar mass of the major peroxyacyl nitrate, peroxyacetyl nitrate, is 118.03 g/mol.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_forwardA piece of magnesium reacts with an aqueous solution of HCl to produce H2 gas. The hydrogen gas is collected over the HCl solution at a temperature of 22.0°C. If the total pressure of the system is 0.957 atm, and the volume of gas collected is 710. mL, what are the partial pressure and the mass of H2 produced? (You may assume that the dissolved HCl has no effect on the vapor pressure of water, which is 19.8 torr at 22.0°C.) partial pressure Massarrow_forwardA piece of magnesium reacts with an aqueous solution of HCl to produce H2 gas. The hydrogen gas is collected over the HCl solution at a temperature of 22.0°C. If the total pressure of the system is 0.965 atm, and the volume of gas collected is 780. mL, what are the partial pressure and the mass of H2 produced? (You may assume that the dissolved HCl has no effect on the vapor pressure of water, which is 19.8 torr at 22.0°C.)arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
- Chemistry: Principles and PracticeChemistryISBN:9780534420123Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward MercerPublisher:Cengage LearningChemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage LearningIntroduction to General, Organic and BiochemistryChemistryISBN:9781285869759Author:Frederick A. Bettelheim, William H. Brown, Mary K. Campbell, Shawn O. Farrell, Omar TorresPublisher:Cengage Learning
- Introductory Chemistry: A FoundationChemistryISBN:9781337399425Author:Steven S. Zumdahl, Donald J. DeCostePublisher:Cengage LearningChemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry: Principles and Practice
Chemistry
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
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
Introductory Chemistry: A Foundation
Chemistry
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning