Physical Chemistry
2nd Edition
ISBN: 9781133958437
Author: Ball, David W. (david Warren), BAER, Tomas
Publisher: Wadsworth Cengage Learning,
expand_more
expand_more
format_list_bulleted
Videos
Textbook Question
Chapter 20, Problem 20.87E
Pyrolysis involves heating compounds to break them into smaller molecules, and typically involves free-radical chain reactions. Pyrolysis of crude oil fractions is a common method of making smaller hydrocarbons from large-chain hydrocarbons. Pyrolysis of ethane,
Expert Solution & Answer
Want to see the full answer?
Check out a sample textbook solution
Students have asked these similar questions
Combustion of glucose (
C6H12O6
) is the main source of energy for animal cells:
C6H12O6
(
s
)
+ 6O2
(
g
)
→ 6CO2
(
g
)
+ 6H2O
(
l
)
=ΔGrxn37°C−2872.kJ
This energy is generally stored as
ATP
(adenosine triphosphate) molecules, which can release it when convenient by hydrolysis ("water-assisted decomposition") into
ADP
(adenosine diphosphate) molecules and a phosphate anion, often given the symbol
Pi
in biochemistry:
ATP
(
aq
)
→ ADP
(
aq
)
+ Pi
(
aq
)
=ΔGrxn−35 to 70kJ
The actual amount of free energy released by the hydrolysis of
ATP
varies, depending on the exact conditions inside the cell.
Suppose under certain conditions hydrolysis of
ATP
actually releases
−51.3/kJmol
. Calculate the maximum number of
ATP
s that could be created from
ADPs
and
Pi
by the combustion of a molecule of glucose. Your answer must be a whole number.
There is great excess of H2O in this reaction.
In glycolysis, glucose is broken down to yield energy. If the equilibrium constant of the isomerization of glucose-6-phosphate to fructose-6-phosphate is 0.5, would this reaction proceed in the forward or reverse direction? What is the free energy of the reaction? Using standard conditions (1 M) as an initial state, what are the equilibrium concentrations?
Chapter 20 Solutions
Physical Chemistry
Ch. 20 - Prob. 20.1ECh. 20 - The oxidation-reduction reaction between iron...Ch. 20 - The oxidation-reduction reaction between iron...Ch. 20 - The rate of the reaction...Ch. 20 - For a certain reaction between NO and O2, the rate...Ch. 20 - For a reaction between SO2 and Cl2, the rate law...Ch. 20 - Consider the chemical reaction A+B+Cproducts...Ch. 20 - For the chemical reaction...Ch. 20 - Explain how a species might be part of a rate law...Ch. 20 - Refer to Example 20.2 and explain whether any...
Ch. 20 - Rate law experiments dont always give data in the...Ch. 20 - Prob. 20.12ECh. 20 - What must the units on k be for the following rate...Ch. 20 - What must the units on k be for the following rate...Ch. 20 - The reaction 2O33O2 has first-order kinetics and a...Ch. 20 - Digestive processes are first-order processes. The...Ch. 20 - Prob. 20.18ECh. 20 - Derive equation 20.15.Ch. 20 - Prob. 20.20ECh. 20 - To a very good approximation, the cooling of a hot...Ch. 20 - Assume that thermal decomposition of mercuric...Ch. 20 - Prob. 20.23ECh. 20 - Prob. 20.24ECh. 20 - Derive equation 20.22.Ch. 20 - a Write a rate law and an integrated rate law for...Ch. 20 - Derive an expression for the half-life of a a...Ch. 20 - Prob. 20.28ECh. 20 - Rewrite equation 20.27 so that it has the form of...Ch. 20 - One can also define a third-life, t1/3, which is...Ch. 20 - The decomposition of NH3: 2NH3N2+3H2 is a...Ch. 20 - Prob. 20.32ECh. 20 - Prob. 20.33ECh. 20 - When ionic compounds crystallize from a...Ch. 20 - An aqueous reaction that uses the solvent H2O as a...Ch. 20 - The rate law for the reaction...Ch. 20 - If a reaction has the same rate constant, what...Ch. 20 - List at least four experimentally determined...Ch. 20 - Prob. 20.39ECh. 20 - Prob. 20.40ECh. 20 - Prob. 20.41ECh. 20 - Prob. 20.42ECh. 20 - What is the value of the equilibrium constant of a...Ch. 20 - Prob. 20.44ECh. 20 - Prob. 20.45ECh. 20 - Show how equation 20.33 reduces to a simpler form...Ch. 20 - Write expressions like equation 20.37 for a set of...Ch. 20 - Prob. 20.48ECh. 20 - Prob. 20.49ECh. 20 - Prob. 20.50ECh. 20 - Prob. 20.51ECh. 20 - Prob. 20.52ECh. 20 - Prob. 20.53ECh. 20 - Prob. 20.54ECh. 20 - For what values of time, t, will 210Bi and 206Pb...Ch. 20 - Prob. 20.56ECh. 20 - An interesting pair of consecutive reactions...Ch. 20 - Find limiting forms of equation 20.47 for a k1>>k2...Ch. 20 - Prob. 20.59ECh. 20 - Prob. 20.60ECh. 20 - Prob. 20.61ECh. 20 - Prob. 20.62ECh. 20 - At room temperature (22C), the rate constant for...Ch. 20 - Recently, researchers studying the kinetics of...Ch. 20 - A reaction has k=1.771061/(Ms) at 25.0C and an...Ch. 20 - Prob. 20.66ECh. 20 - Prob. 20.67ECh. 20 - Prob. 20.68ECh. 20 - Nitric oxide, NO, is known to break down ozone,...Ch. 20 - a Suggest a mechanism for the bromination of...Ch. 20 - Prob. 20.71ECh. 20 - Prob. 20.72ECh. 20 - Determine a rate law for the chlorination of...Ch. 20 - Determine a rate law for the chlorination of...Ch. 20 - A proposed mechanism for the gas-phase...Ch. 20 - Prob. 20.76ECh. 20 - The nitration of methanol, CH3OH, by nitrous acid...Ch. 20 - Prob. 20.78ECh. 20 - Many gas-phase reactions require some inert body,...Ch. 20 - Prob. 20.80ECh. 20 - Carbonic anhydrase, an enzyme whose substrate is...Ch. 20 - Show that another form of the Michaelis-Menten...Ch. 20 - Prob. 20.83ECh. 20 - Prob. 20.84ECh. 20 - Prob. 20.85ECh. 20 - Prob. 20.86ECh. 20 - Pyrolysis involves heating compounds to break them...Ch. 20 - Prob. 20.88ECh. 20 - Label the elementary processes for the reaction...Ch. 20 - Prob. 20.90ECh. 20 - What are the rate laws of mechanisms 1 and 2 for...Ch. 20 - Estimate G for an elementary process whose rate...Ch. 20 - Prob. 20.93ECh. 20 - Prob. 20.94ECh. 20 - Prob. 20.95ECh. 20 - For the following two reactions H+Cl2HCl+Cl...Ch. 20 - Prob. 20.97ECh. 20 - Prob. 20.98ECh. 20 - Prob. 20.99ECh. 20 - Consider a reaction that has two parallel pathways...Ch. 20 - Consider a set of first-order consecutive...Ch. 20 - Prob. 20.102E
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
- Amoxicillin is an antibiotic packaged as a powder. When it is used to treat babies and small animals, the pharmacist or veterinarian must suspend it in water, so that it can be administered orally with a medicine dropper. The label says to dispose of unused suspension after 14 days. It also points out that refrigeration is required. In the context of this chapter, what is implied in the latter two statements?arrow_forwardA supersaturated solution of sucrose (C12H22O11) is made by dissolving sucrose in hot water and slowly letting the solution cool to room temperature. After a long time, the excess sucrose crystallizes out of the solution. Indicate whether each of the following statements is true or false: After the excess sucrose has crystallized out, the rate of sucrose molecules leaving the surface of the crystals to be hydrated by water is equal to the rate of sucrose molecules in water attaching to the surface of the crystals.arrow_forwardFor the reaction 2Fe2O3⟶4Fe+3O2 Δ?∘rxn=+824.2 kJ/mol the decomposition of 39.039.0 g of Fe2O3 results in a) the release of 16100 kJ16100 kJ of heat. b) the absorption of 201 kJ201 kJ of heat. c) the absorption of 16100 kJ16100 kJ of heat. d) the absorption of 101 kJ101 kJ of heat. e) the release of 201 kJ201 kJ of heat. f) the release of 101 kJ101 kJ of heat.arrow_forward
- Monochloroethane (C2H5Cl) can be produced by the direct reaction of ethane gas (C2H6) with chlorine gas or by the reaction of ethylene gas (C2H4) with hydrogen chloride gas. The second reaction gives almost a 100% yield of pure C2H5Cl at a rapid rate without catalysis. The first method requires light as an energy source or the reaction would not occur. Yet G for the first reaction is considerably more negative than G for the second reaction. Explain how this can be so.arrow_forwardAnother step in the metabolism of glucose, which occurs after the formation of glucose6-phosphate, is the conversion of fructose6-phosphate to fructose1,6-bisphosphate(bis meanstwo): Fructose6-phosphate(aq) + H2PO4(aq) fructose l,6-bisphosphate(aq) + H2O() + H+(aq) (a) This reaction has a Gibbs free energy change of +16.7 kJ/mol of fructose6-phosphate. Is it endergonic or exergonic? (b) Write the equation for the formation of 1 mol ADP fromATR for which rG = 30.5 kJ/mol. (c) Couple these two reactions to get an exergonic process;write its overall chemical equation, and calculate theGibbs free energy change.arrow_forwardUse data from Appendix IIB to calculate ΔS∘rxnΔSrxn∘ for each of the reactions given. 3NO2(g)+H2O(l)→2HNO3(aq)+NO(g) Express your answer as an integer. ΔS∘rxn=____________________J/Karrow_forward
- What is the difference between KD and KA? in relation to “Law of Mass Action"arrow_forwardThe combustion of glucose is given by the reaction C6H12O6 (s) + 6O2 →6H2O(l)+6CO2 (g) The heats of formation are: C6H12O6 (s):-1274.5 kJ/mol; H2O(l):-285.8 kJ/mol; CO2 (g):-393.5 kJ/mol. Calculate ΔrH0 for the combustion of glucose?arrow_forwardBalance the equation and write the reaction quotient expression, Qc, for the following synthesis of carbon disulfide, CS2: CH4(g) + H2S(g) ⇌ CS2(g) + H2(g)arrow_forward
- The conversion of natural gas, which is mostly methane,into products that contain two or more carbon atoms, suchas ethane (C2H6), is a very important industrial chemicalprocess. In principle, methane can be converted into ethaneand hydrogen: 2 CH4(g)----->C2H6(g) + H2(g) In practice, this reaction is carried out in the presence ofoxygen: 2 CH4(g) + 12O2(g)---->C2H6(g) + H2O(g) (a) Calculate K for these reactionsat 25 °C and 500 °C. (b) Is the difference in ΔG° forthe two reactions due primarily to the enthalpy term (ΔH)or the entropy term 1-TΔS2? (c) Explain how the precedingreactions are an example of driving a nonspontaneousreaction, (d) The reaction of CH4 and O2 to form C2H6 and H2O must be carried out carefully to avoid a competingreaction. What is the most likely competing reaction? Cells use the hydrolysis of adenosine triphosphate (ATP)arrow_forwardThe conversion of natural gas, which is mostly methane,into products that contain two or more carbon atoms, suchas ethane (C2H6), is a very important industrial chemicalprocess. In principle, methane can be converted into ethaneand hydrogen: 2 CH4(g)----->C2H6(g) + H2(g) In practice, this reaction is carried out in the presence ofoxygen: 2 CH4(g) + 12O2(g)---->C2H6(g) + H2O(g) (a) Calculate K for these reactionsat 25 °C and 500 °C. (b) Is the difference in ΔG° forthe two reactions due primarily to the enthalpy term (ΔH)or the entropy term 1-TΔS2? (c) Explain how the precedingreactions are an example of driving a nonspontaneousreaction, (d) The reaction of CH4 and O2 to form C2H6 and H2O must be carried out carefully to avoid a competingreaction. What is the most likely competing reaction?arrow_forwardThe following reversible enzymatic reaction occurs in many areas of the body, but especially in red blood cells. The conversion of water and carbon dioxide into bicarbonate and hydrogen ions occurs through the action of an enzyme called carbonic anhydrase. Use the Law of Mass Action to predict which direction this equation will go under different circumstances. CO2 + H2O ↔ H+ + HCO3- Hyperventilating would increase the loss of carbon dioxide (CO2) from the blood. In what direction would the reaction above go in order to restore equilibrium? Left or right?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: 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
Chemistry: An Atoms First ApproachChemistryISBN:9781305079243Author:Steven S. Zumdahl, Susan A. ZumdahlPublisher:Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
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
Chemistry: An Atoms First Approach
Chemistry
ISBN:9781305079243
Author:Steven S. Zumdahl, Susan A. Zumdahl
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