Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN: 9781938168390
Author: Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher: OpenStax
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 12, Problem 8E
Explain why an egg cooks move slowly in boiling water in Denver than in New York City. (Hint: Consider the effect 0f temperature on reaction rate and the effect of pressure on boiling point.)
Expert Solution & Answer
Trending nowThis is a popular solution!
Students have asked these similar questions
The following reaction is carried out at 25.0 °C and 1.00 atm:
2NO(g) + O2(g) →→ 2NO2(g)
AH0 kJmol-1
Sº JK-¹mol-1
NO (g)
-110.525
197.674
NO₂ (g)
-393.509
213.74
O₂ (g)
0.00
205.0
Using the data in the table:
• Calculate the enthalpy of reaction, A₁H, for the reaction:
mol-1
• Calculate the entropy change, ASº, for the reaction:
• Calculate AGO for the reaction:
kJ mol-1
Is this reaction spontaneous or not spontaneous at this temperature and
pressure?
kJ
JK-1 mol-1
Under equilibirum conditions at 565.3 K, [H2]=.06906 mol/L, [CO]=.01515 mol/L, [Ch3OH]= .0401 mol/L. What is value of Kc for this reaction at 565.3 K?
(Data attached in picture)
KINETICS AND EQUILIBRIUM
Using Le Chatelier's Principle to predict the result of changing...
Nitrogen and hydrogen react to form ammonia, like this:
N₂(g) +3 H₂(g) →2NH₂(g)
The reaction is exothermic. Suppose a mixture of N₂, H₂ and NH3 has come to equilibrium in a closed reaction vessel. Predict what change, if any, the
perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left.
perturbation
change in composition
The temperature is raised. The pressure of NH3 will ?
The temperature is
lowered.
The pressure of N₂ will
?
?
go up.
go down.
not change.
shift in equilibrium
to the right
to the left
O (none)
to the right
to the left
O (none)
X
1/5
Chapter 12 Solutions
Chemistry by OpenStax (2015-05-04)
Ch. 12 - What is the difference between average rate,...Ch. 12 - Ozone decomposes to oxygen according to the...Ch. 12 - In the nuclear industry, chlorine trifluoride is...Ch. 12 - A study of the rate of dimerization of C4H6 gave...Ch. 12 - A study of the rate of the reaction represented as...Ch. 12 - Consider the following reaction in aqueous...Ch. 12 - Describe the effect of each of the following on...Ch. 12 - Explain why an egg cooks move slowly in boiling...Ch. 12 - Go to the PhET Reactions and change to Angled...Ch. 12 - In the PhET Reactions tab to observe how multiple...
Ch. 12 - In the PhET Reactions under Options. (a) Leave...Ch. 12 - How do the rate of a reaction and its rate...Ch. 12 - Doubling the concentration of a reactant increases...Ch. 12 - Tripling the concentration of a reactant increases...Ch. 12 - How much and in what direction will each of the...Ch. 12 - How will each of the following affect the rate of...Ch. 12 - Regular ?ights of supersonic aircraft in the...Ch. 12 - Radioactive phosphorus is used in the study of...Ch. 12 - The rate constant for the radioactive decay of 14C...Ch. 12 - The decomposition of acetaldehyde is a second...Ch. 12 - Alcohol is removed from the bloodstream by a...Ch. 12 - Under certain conditions the decomposition of...Ch. 12 - Nitrosyl chloride, NOCI, decomposes to NO and CI2....Ch. 12 - From the following data, determine the rate...Ch. 12 - Nitrogen monoxide reacts with chlorine according...Ch. 12 - Hydrogen reacts with nitrogen monoxide to form...Ch. 12 - For the reaction AB+C, the following data were...Ch. 12 - For the reaction QW+X, the following data were...Ch. 12 - The rate constant for the ?rst-order decomposition...Ch. 12 - The annual production of HNO3 in 2013 was 60...Ch. 12 - The following data have been determined for the...Ch. 12 - Describe how graphical methods can be used to...Ch. 12 - Use the data provided to graphically determine the...Ch. 12 - Use the data provided in a graphical method to...Ch. 12 - Pure ozone decomposes slowly to oxygen, 2O33O2(g)....Ch. 12 - From the given data, use a graphical method to...Ch. 12 - What is the half-life for the first-order decay of...Ch. 12 - What is the half-life for the first-order decay of...Ch. 12 - What is the half-life for the decomposition of...Ch. 12 - What is the half-life for the decomposition of O3...Ch. 12 - The reaction of compound A to give compounds C and...Ch. 12 - The half-life of a reaction of compound A to give...Ch. 12 - Some bacteria are resistant to the antibiotic...Ch. 12 - Both technetium-99 and thallium-201 are used to...Ch. 12 - There are two molecules with the formula C3H6...Ch. 12 - Fluorine-18 is a radioactive isotope that decays...Ch. 12 - Suppose that the half-life of steroids taken by an...Ch. 12 - Recently, the skeleton of King Richard III was...Ch. 12 - Nitroglycerine is an extremely sensitive...Ch. 12 - For the past 10 years, the unsaturated hydrocarbon...Ch. 12 - Chemical reactions occur when reactants collide....Ch. 12 - When every collision between reactants leads to a...Ch. 12 - What is the activation energy of a reaction, and...Ch. 12 - Account for the relationship between the rate of a...Ch. 12 - Describe how graphical methods can be used to...Ch. 12 - How does an increase in temperature affect rate of...Ch. 12 - The rate of a certain reaction doubles for every...Ch. 12 - In an experiment, a sample of NaClO3 was 90%...Ch. 12 - The rate constant at 325 C for the decomposition...Ch. 12 - The rate constant for the decomposition of...Ch. 12 - An elevated level of the enzyme alkaline...Ch. 12 - In terms of collision theory, to which of the...Ch. 12 - Hydrogen iodide, HI, decomposes in the gas phase...Ch. 12 - The element Co exists in two oxidation states,...Ch. 12 - The hydrolysis of the sugar sucrose to the sugars...Ch. 12 - Use the PhET Reactions Single collision" tab of...Ch. 12 - Use the PhET Reactions Single collision tab of the...Ch. 12 - Why awe elementary reactions involving three or...Ch. 12 - In general, can we predict the effect of doubling...Ch. 12 - Define these terms: (a) unimolecular reaction (b)...Ch. 12 - What is the rate equation for the elementary...Ch. 12 - Given the following reactions and the...Ch. 12 - Write the rate equation for each of the following...Ch. 12 - Nitrogen (Il) oxide, NO, reacts with hydrogen, H2,...Ch. 12 - Experiments were conducted to study the rate of...Ch. 12 - The reaction of CO with CI2 gives phosgene...Ch. 12 - . Account for the increase in reaction rate...Ch. 12 - Compare the functions of homogeneous and...Ch. 12 - Consider this scenario and answer the following...Ch. 12 - For each of the following pairs of reaction...Ch. 12 - For each of the following pairs of reaction...Ch. 12 - For each of the following reaction diagrams,...Ch. 12 - For each of the following reaction diagrams,...Ch. 12 - Based on the diagrams in Exercise 12.83, which of...Ch. 12 - Based on the diagram in Exercise 12.83, which of...
Additional Science Textbook Solutions
Find more solutions based on key concepts
(a) What is the efficiency of an out-of-condition professor who does 2.10105J of useful work while metabolizing...
College Physics
In the following diagram, the white spheres represent hydrogen atoms and the blue Sphere represent the nitrogen...
Chemistry: The Central Science (13th Edition)
Determine the Coulombic and exchange energies for the following states, and determinewhich state is favored (ha...
Inorganic Chemistry
Write a balanced chemical equation for each chemical reaction. a. Solid copper reacts with solid sulfur to form...
Introductory Chemistry (6th Edition)
The reaction of tert-butyl chloride with methanol (CH3)3CCl + CH3OH (CH3)3COCH3 + HCl tert butyl chloride met...
Organic Chemistry (9th Edition)
A 50.0 g piece of iron at 152°C is dropped into 20.0 g H2O(l) at 89 °C in an open, thermally insulated containe...
General Chemistry: Principles and Modern Applications (11th Edition)
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
- 5.12. True or false: If all the partial pressures of reactants and products drop by half, the value of Q drops by half. Give an example of a chemical reaction to support your answer.arrow_forwardWhy are there no changes specified for Ni in Exercise 13.61, part (f)? What property of Ni does change?arrow_forwardExplain why the development of a vapor pressure above a liquid in a closed container represents an equilibrium. What are the opposing processes? How do we recognize when the system has reached a state of equilibrium?arrow_forward
- Determine the Ke if the K₂ = 2.89 for the reaction below at 327 °C. 2 NO2 (g) N₂04 (g) Recall that Kp = K (RT)Anarrow_forwardUsing Le Chatelier's Principle to predict the result of changing... Ammonia and oxygen react to form nitrogen and water, like this: 4NH3 (g)+30₂ (g) 2N₂(g)+6H₂O(g) Suppose a mixture of NH3, O2, N₂ and H₂O has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation Some NH3 is added. Some H₂O is removed. change in composition The pressure of O₂ will The pressure of N₂ will The pressure of NH3 will ? ? ? shift in equilibrium to the right to the left O (none) to the right to the leftarrow_forwardRates of reaction are found to increase with temperature. Sketch a labelled diagram that shows the distribution of molecular energies at two different temperatures. State two theories that explain the effect of temperature increase on rates of reaction.arrow_forward
- Determine Kandk,at 298 K for the reaction: NOBR(g) = % N2(g) + O2(g) + % Br2(g) from the following information at 298 K: NO(9) = % N2(g) + % O2(a) Ke = 1.55 x 1015 % NO(g) + % Br2(g) = % NOBr(a) Kp = 2.63 Type your answers below. Note: If answering in scientific notation, type your answer this way: 1.23 x 1045 → type 1.23e45 ANSWERS: Kc = Kp =arrow_forwardC6H5CHO reacts with H₂ to form C6H5CH₂OH. The equilibrium constant, Kp, for this reaction is 1.79 at 523 K. C6H5CHO(g) + H₂(g) 2CH₂CH₂OH(g) The standard enthalpy change for this reaction (AHº) is -55.5 kJ/mol. (a) Predict the effect on the production of C6H₂CH₂OH when the temperature of the equilibrium system is increased. ŵ (b) Use the van't Hoff equation to estimate the equilibrium constant for this reaction at 632 K. Kp at 632 K =arrow_forward• Consider the following reaction: 3 Fe(s) + 4 H₂O(g) ↔ Fe3O4(s) + 4 H₂(g) At 900 °C, Kc for the reaction is 5.1. If 0.050 mol H₂O(g) and 0.100 mole Fe(s) are placed in a 1.0 L container at 900 °C, how many grams of Fe₂O4 are present when equilibrium is establishedarrow_forward
- 3.) For the following equilibrium reaction2NO2(g) ↔N2O4(g) + Δlook in the Tro text to see what LeChatelier's principle states about gases. Assume that the reaction occurs in an enclosed movable piston. [Hint: remember that PV=nRT] a.) The pressure of the reaction is increased. b.) The volume of the reaction is decreased. c.) The volume of the reaction is increased.arrow_forwardAt 455 K, this reaction has a Ke value of 0.0390. 2 X(g) + 2 Y(g) = Z(g) Calculate Kp at 455 K. Note that the pressure is in units of atmosphere (atm).arrow_forwardMethane and chlorine react to form chloroform and hydrogen chloride, like this: CH (g)+3Cl,(g) → CHCI3(g)+3HCI(g) The reaction is exothermic. Suppose a mixture of CH, Cl,, CHCI, and HCl has come to equilibrium in a closed reaction vessel. Predict what change, if any, the perturbations in the table below will cause in the composition of the mixture in the vessel. Also decide whether the equilibrium shifts to the right or left. perturbation change in composition shift in equilibrium O to the right The temperature is lowered. O to the left The pressure of CHA will O (none) O to the right O to the left The temperature is raised. The pressure of CHCI3 will ? O (none) Check O 2021 McGraw-Hill Education, All Rights Reserved Terms of Use Pacy Explanation hparrow_forward
arrow_back_ios
SEE MORE QUESTIONS
arrow_forward_ios
Recommended textbooks for you
World of Chemistry, 3rd editionChemistryISBN:9781133109655Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCostePublisher:Brooks / Cole / Cengage Learning
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
Principles of Modern ChemistryChemistryISBN:9781305079113Author:David W. Oxtoby, H. Pat Gillis, Laurie J. ButlerPublisher:Cengage Learning
Chemistry: The Molecular ScienceChemistryISBN:9781285199047Author:John W. Moore, Conrad L. StanitskiPublisher:Cengage Learning
ChemistryChemistryISBN:9781305957404Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCostePublisher:Cengage Learning
World of Chemistry, 3rd edition
Chemistry
ISBN:9781133109655
Author:Steven S. Zumdahl, Susan L. Zumdahl, Donald J. DeCoste
Publisher:Brooks / Cole / Cengage Learning
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
Principles of Modern Chemistry
Chemistry
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:9781285199047
Author:John W. Moore, Conrad L. Stanitski
Publisher:Cengage Learning
Chemistry
Chemistry
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Cengage Learning
Kinetics: Chemistry's Demolition Derby - Crash Course Chemistry #32; Author: Crash Course;https://www.youtube.com/watch?v=7qOFtL3VEBc;License: Standard YouTube License, CC-BY