CHEMISTRY-TEXT
8th Edition
ISBN: 9780134856230
Author: Robinson
Publisher: PEARSON
expand_more
expand_more
format_list_bulleted
Concept explainers
Videos
Textbook Question
Chapter 11, Problem 11.10P
A fire extinguisher containing carbon dioxide has a pressure of 70 atm at 75 °F. What phase of CO2 is present in the tank?
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
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?
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 801.1 mL aqueous solution of 628.5 mM Na2S is combined with 100.0 mL of an aqueous HCl solution whose HCl concentration is not known. The reaction produces 4.126 L of H2S gas at a pressure of 1.00 atm and a temperature of 35.93∘C. There are sulfide ions still present in the solution after the reaction is complete. What was the concentration of HCl in the original HCl solution? Express your answer in units of molar (M) using at least three significant digits.
Chapter 11 Solutions
CHEMISTRY-TEXT
Ch. 11 - Prob. 11.1PCh. 11 - The normal boiling point of water is 100.0 C, and...Ch. 11 - PRACTICE 11.1 The boiling point of ethanol is 78.4...Ch. 11 - APPLY 11.2 Chloroform CHCl3 has Hvap=29.2kJ/mol...Ch. 11 - How much heat is required to convert15.0 g of...Ch. 11 - APPLY 11.4 What is the sign and magnitude of q...Ch. 11 - Look at the phase diagram of H2O in Figure 11.7,...Ch. 11 - Prob. 11.8ACh. 11 - Why was a new solvent needed for extracting...Ch. 11 - A fire extinguisher containing carbon dioxide has...
Ch. 11 - Look at the phase diagram of CO2 in Figure11.13,...Ch. 11 - Liquid carbon dioxide is also used as non-toxic...Ch. 11 - For the phase transition CO2(s)CO2(g), predict the...Ch. 11 - A sample of supercritical carbon dioxide was...Ch. 11 - Assume that you have a liquid in a cylinder...Ch. 11 - The phase diagram of a substance is shown below....Ch. 11 - Prob. 11.17CPCh. 11 - Prob. 11.18CPCh. 11 - The following compound undergoes a phase...Ch. 11 - A magnetized needle gently placed on the surface...Ch. 11 - Water flows quickly through the narrow neck of a...Ch. 11 - Predict which substance in each pair has the...Ch. 11 - Prob. 11.23SPCh. 11 - The chemical structure for oleic acid, the primary...Ch. 11 - Prob. 11.25SPCh. 11 - Prob. 11.26SPCh. 11 - The vapor pressure of SiCI4 is 100 mm Hg at 5.4 C,...Ch. 11 - What is the vapor pressure of CS2 in mm Hg at 20.0...Ch. 11 - What is the vapor pressure of SiCI4 in mm Hg at...Ch. 11 - Dichloromethane, CH2CI2, is an organic solvent...Ch. 11 - Prob. 11.31SPCh. 11 - Use the plot you made in Problem 11.30 to find a...Ch. 11 - Prob. 11.33SPCh. 11 - Prob. 11.34SPCh. 11 - Prob. 11.35SPCh. 11 - Prob. 11.36SPCh. 11 - Acetone,acommon laboratorysolvent,has...Ch. 11 - Why is Hvap usually larger than Hfusion ?Ch. 11 - Why is the heat of sublimation, Hsubl, equal to...Ch. 11 - Naphthalene, better known as "mothballs," has bp =...Ch. 11 - Prob. 11.41SPCh. 11 - Prob. 11.42SPCh. 11 - Prob. 11.43SPCh. 11 - Prob. 11.44SPCh. 11 - Prob. 11.45SPCh. 11 - How much energy in kilojoules is needed to heat...Ch. 11 - Prob. 11.47SPCh. 11 - How much energy in kilojoules is released when...Ch. 11 - How much energy in kilojoules is released when...Ch. 11 - Prob. 11.50SPCh. 11 - Prob. 11.51SPCh. 11 - Prob. 11.52SPCh. 11 - Prob. 11.53SPCh. 11 - Prob. 11.54SPCh. 11 - Look at the phase diagram of H2O in Figure 11.7,...Ch. 11 - Prob. 11.56SPCh. 11 - Oxygen has Tt=54.3K,Pt=1.14mmHg,Tc=154.6K, and...Ch. 11 - Prob. 11.58SPCh. 11 - Prob. 11.59SPCh. 11 - Prob. 11.60SPCh. 11 - Prob. 11.61SPCh. 11 - Benzene has a melting point of 5.53 C and a...Ch. 11 - Prob. 11.63SPCh. 11 - How many phase transitions did you pass through in...Ch. 11 - Prob. 11.65SPCh. 11 - Prob. 11.66SPCh. 11 - Prob. 11.67SPCh. 11 - Prob. 11.68SPCh. 11 - Prob. 11.69SPCh. 11 - Prob. 11.70SPCh. 11 - Prob. 11.71SPCh. 11 - Prob. 11.72SPCh. 11 - Prob. 11.73SPCh. 11 - For each of the following substances, identify the...Ch. 11 - The chlorofluorocarbon refrigerant...Ch. 11 - Prob. 11.76MPCh. 11 - Prob. 11.77MP
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
- What possible uses exist for the natural gas liquids that are removed from natural gas during its processing?arrow_forwardWhat is the mole fraction of H 2 S O 4 in a solution containingthe percentage of sulfuric acid and water shownin Figure 14.25?arrow_forwardA 1,365.8 mL aqueous solution of 407.9 mM Na2S is combined with 100.0 mL of an aqueous HCl solution whose HCl concentration is not known. The reaction produces 3.36 L of H2S gas at a pressure of 1.00 atm and a temperature of 11.88∘C. There is some Na2S remaining after the reaction is complete. What is the concentration of sulfide ions in the solution after the reaction has completed? Assume the volumes of the solutions are additive. Express your answer in units of millimolar (mM) using at least three significant digits.arrow_forward
- Part A. Multiple Choice Identify the choice that best completes the statement or answers the question. L·atm R = 0.08206 mol · K 1. At 0.982 atm, the height of mercury in a barometer is 0.746 m. If the mercury were replaced with ethanol, what height of ethanol (in meters) would be supported at this pressure? The densities of Hg and ethanol are 13.5 g/cm³ and 0.789 g/cm³, respectively. а. 0.0436 m b. 0.946 m с. 0.760 m d. 12.8 m е. 13.0 marrow_forwardA 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.arrow_forward● One mole of water weighs 18 g at 4 °C. True Falsearrow_forward
- Consider 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_forward2. A tank was filled with 12 g of oxygen (O2), 73 g of nitrogen (N2) and 4 g of carbon dioxide(CO2). At 25°C the pressure of the tank was 7.5 atm. If the partial pressure of CO2 in the tank is x atm, what is the value of x?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
- How many hypochlorite ions are present in 1.50 gal of bleach solution? (1gal=3.785L) Write the balanced chemical equation for the preparation of bleach. Express your answer as a chemical equation. Identify all of the phases in your answer. How many grams of NaOHare required to produce the sodium hypochlorite for 1.50 gal of bleach? If 165 g of Cl2 is passed through a solution containing 275 g of NaOH and 162 g of sodium hypochlorite is produced, what is the percent yield for the reaction?arrow_forwardEnter your answer in the provided box. A piece of sodium metal reacts completely with water as follows: 2 Na(s)+2H2O(l)->2NaOH(aq)+H2(g)The hydrogen gas generated is collected over water at 23.0\ deg C. The volume of the gas is 291 mL measured at 0.965 atm. Calculate the number of grams of sodium used in the reaction. (The vapor pressure of water at 23.0\deg C=0.027 atm.)arrow_forwardA sample of gas that is (5.160x10^-1) mol is initially at (3.33x10^2) K, (7.2700x10^2) mm Hg, and (8.980x10^0) L. What will be the new temperature (in K) if 0.200 mol of gas are added to this sample and the pressure is changed to (7.630x10^2) mm Hg and the volume is changed to (8.6300x10^0) L?arrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
Chemistry for Engineering StudentsChemistryISBN:9781337398909Author:Lawrence S. Brown, Tom HolmePublisher:Cengage Learning
Chemistry: Matter and ChangeChemistryISBN:9780078746376Author:Dinah Zike, Laurel Dingrando, Nicholas Hainen, Cheryl WistromPublisher:Glencoe/McGraw-Hill School Pub Co
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781133949640Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry & Chemical ReactivityChemistryISBN:9781337399074Author:John C. Kotz, Paul M. Treichel, John Townsend, David TreichelPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
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
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Types of Matter: Elements, Compounds and Mixtures; Author: Professor Dave Explains;https://www.youtube.com/watch?v=dggHWvFJ8Xs;License: Standard YouTube License, CC-BY