The second law of thermodynamics states thatthe entropy of a pure crystalline substance is zero at absolute zeroA.OB AS = grev/T at constant temperaturefor any spontaneous process, the entropy of the universe increasesOC.the entropy of the universe is always constantAE = q +w

The second law of thermodynamics predicts the reversibility of a process. According to this law, the…

The second law of thermodynamics states that the entropy of a pure crystalline substance is zero at absolute zero O A. O B. AS = qrev/T at constant temperature for any spontaneous process, the entropy of the universe increases OC. the entropy of the universe is always constant AE = q + w OE.

The second law of thermodynamics states that the entropy of a pure crystalline substance is zero at absolute zero O A. O B. AS = qrev/T at constant temperature for any spontaneous process, the entropy of the universe increases OC. the entropy of the universe is always constant AE = q + w OE.

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 21Q: The third law of thermodynamics states that the entropy of a perfect crystal at 0 K is zero. In...

See similar textbooks

Related questions

Q: enthalpy

Q: Two objects A and B are initially at temperatures TA-350 K a two objects. If over a short interval…

A: According to the question, two objects A and B are initially at the temperature Ta = 350 K and Tb =…

Q: Consider the reaction CO(g) + Cl2(g)COCl2(g) Using standard thermodynamic data at 298K, calculate…

Q: Q4) A cube of ice of mass 100 git put into a gloss of water at just above 0°C. When the ite melts,…

A: Given, Heat absorbed in fusion of 100 g ice = 33KJ. Temperature of the system = 0°C. And entropy…

Q: Estimate the temperatures at which the following stratospheric reactions become spontaneous under…

A: Given: A thermodynamic data

Q: 5. For a pure substance a. Derive the following expression пк T. b. How does the molar entropy…

Q: A system undergoes a transformation for which ASsys 0. The transformation will definitely be…

A: Gibbs free energy : ΔG = ΔH - ΔS For a process to be spontaneous, ΔG < 0 ΔGsys < 0 ΔH -TΔSsys…

Q: For the isothermal expansion of a gas into a vacuum,ΔE = 0, q = 0, and w = 0. (a) Is this a…

A: (a) The spontaneous process is the process which starts on its own or initiate without any external…

Q: For water, ΔHfusion = 6.02 kJ/mol and ΔHvap = 40.65 kJ/mol. If 0.250 moles of water vaporizes at…

A: ∆Ssurrounding = - ∆Ssystem. ∆Ssurrounding = - ∆Hvaporization / Tboiling.

Q: Under standard conditions the absolute entropy of liquid water is (H2O(l)) = 69.91 J K-1 mol-1 .…

Q: Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy…

Q: Use the information provided in the table below to calculate the change in entropy of the universe…

A: To solve this problem we have to first calculate ∆Ssys and ∆Ssurr As we know that ∆Suniv =…

Q: Many of the biological reactions that are essential for the formation and maintenance of highly…

A: The correct answer is given below

Q: Consider the reaction2CO(g) + O2(g)2CO2(g)Using standard thermodynamic data at 298K, calculate the…

A: Given, 2.27 moles of CO(g)

Q: Consider the following reaction under the standard state. 2 NO3 (g) = 2 NO2 (g) + 02 (g) The…

Q: Consider the reaction: NH4Cl(aq)NH3(g) + HCl(aq) Using standard thermodynamic data at 298K,…

A: Interpretation - To determine the entropy change for the surroundings when 1.76 moles of NH4Cl(aq)…

Q: A substance has a molar specific heat, cV,m=4.00 J K-1mol-1and a molar mass, M=10.0 g/mol. A 100.0 g…

A: Given : mass of sample 1 and 2 and molar mass of sample and molar specific heat. To find: final…

Q: 4-entro Consider the reaction 2NO(g) + O2(g) 2NO2(g) Using standard thermodynamic data at 298K,…

A: given Moles of No reacted = 1.77 moles

Q: Given: H2O(l) → H2O(s) ΔH° = –6.02 kJ at 273K Calculate the entropy change of the…

A: Given : ΔH° = –6.02 kJ (1kJ = 1000 J) ΔH° = –6.02 x 10 3 J (1kJ = 1000 J) Temperature (T) = 0° =…

Q: Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy…

Q: The nonspontaneous reactionD + E → Fdecreases the system entropy by 51 J/(K·mol). What is…

A: Gibbs free energy equation is given by,

Q: The heat capacity of trichloromethane in the range 240 K to 330 K is given by the equation: Cp,m (J…

Q: Briefly: a. What does this say about an ideal gas? (@E/®V)† = 0 b. How do we know it is true? Either…

A: Internal energy is the energy associated with the random, disordered motion of molecules. Entropy is…

Q: Which statements are true? O ASsys = -ASurr for ice melting at room temperature. O All other…

A: The correct statements are:

Q: A substance has a molar specific heat, cV,m=4.00 J K-1mol-1and a molar mass, M=10.0 g/mol. A 100.0 g…

A: Given : Intial temperature of sample 1= 250 K. Initial temperature of sample 2 = 400…

Q: (a) (i) What are the thermodynamic quantities of a system that affect the amount and sign of the…

A: SOLUTION: Step 1: (a). (i). For a closed system, with matter transfer excluded, the changes in the…

Q: The entropy of potassium peroxide, (K2O2 ) is 113.1 J/K. If you have 29.76 g of K2O2 what is the…

Q: Which set of values is thermodynamically AG/KJ >0 >0 0 impossible? AS/J K¹ >0 0 <0 Keq MAAAB

A: Given reaction is : Which set of values is thermodynamically impossible ? Table is : Here, ΔG =…

Q: 21 g of nitrogen gas ( M = 28 g/mol) exerts a pressure of 1.75 atm in a 22.5 L tank What is the…

A: “Since you have asked multiple questions, we will solve the first question for you. If you want any…

Q: Cv aT3 >T Te Figure 2: Heat capacity at constant volume of a substance. The heat capacity at…

A: We have find out entropy and internal energy of a substance.

Q: Consider the reaction: 2H2O(l)2H2(g) + O2(g) Using standard thermodynamic data at 298K, calculate…

Q: What is the entropy change of a gas in J/K (to 2 decimal points) when one mole of a perfect gas…

A: Given that - Number of moles of gas = 1 Initial volume of gas = 0.36 m3 Final volume of gas =…

Q: A heat source generates heat at a rate of 71.0 W (1 W = 1 J/s). How much entropy does this produce…

A: The heat generated by the heat source is = 71.0 W = 71.0 J/s The temperature of the surrounding is =…

Q: The entropy change for the process H2O(s)⟶H2O(l) is 15.2 J/K and requires that the surroundings…

A: Reaction: H2O(s) ⟶ H2O(l) ∆Ssystem = 15.2 J/K ∆H = 38.6 KJ ∆STotal =? T = 76.3 °C = 76.3 + 273.15 =…

Q: Consider the reaction 4-entro 4HCI(g) + O2(g) 2H2O(g) + 2C12(g) Using standard thermodynamic data at…

A: Given moles of HCl reacted = 1.5 moles

Q: Consider a heat engine operating between a high temperature of 127◦C and a low temperature of 27◦C.…

A: If we give energy to the heat engine then some amount of energy will convert into work and some…

Q: When the oxide of generic metal M is heated at 25.0 ∘C, a negligible amount of M is produced.…

Q: The enthalpy for a certain process is 146.4 kJ/mol and the entropy for the process is 463.6 J/K. At…

Q: 4) Consider the isothermal expansion of a 1.00 mol sample of ideal gas at 37 from the initial…

A: Dear student , since you have posted multiple parts questions we are allowed to solve only first…

Q: Calculate the entropy change for the following process. H2O (s, 100 g, -10°C, 1bar) →H2O (s, 100 g,…

Q: When the oxide of generic metal MM is heated at 25.0 ∘C, a negligible amount of MM is produced.…

A: Conversion of graphite to carbon dioxide: a). The chemical equation of coupled process:

Q: (a) Does the entropy of the surroundings increase for spontaneousprocesses? (b) In a particular…

A: Entropy, the measure of a system's thermal energy per unit temperature that is unavailable for doing…

Q: Consider the reaction: 2NO(g) + O2(g)2NO2(g) Using standard absolute entropies at 298K, calculate…

A: The reaction given is, => 2 NO (g) + O2 (g) → 2 NO2 (g) Given: Moles of NO reacting = 2.11 mol.…

Q: Using the thermodynamic information in the ALEKS Data tab, calculate the standard reaction entropy…

A: The reaction given is, => Al2O3 (s) + 3 H2 (g) → 2 Al (s) + 3 H2O (g)

Q: An object at 400 K absorbs 25.0 kJ of heat from the surroundings. What is the change in entropy ΔS…

A: The given data is as follows: The temperature of the object = 400 K The object absorbs heat ∆H= 25.0…

Q: Consider the reaction N2(g) + 3H2(g)- →2NH3(g) Using standard thermodynamic data at 298K, calculate…

A: Please have a look on the solution:

Q: Consider the reaction CO(g) + H20(1)–CO2(g) + H2(g) Using standard thermodynamic data at 298K,…

Q: 1. The heat capacity at 1 atm. pressure of solid magnesium in the temperature rançe from 0 °C to 560…

A: The increase of entropy per g. atom is to be calculated

Q: Exothermic Changes: the system by the surroundings the surroundings. The heat the freedom of motion…

A: Exothermic changes The system looses heat to the surrounding.the heat gain by the surrounding…

Question

The second law of thermodynamics states that
the entropy of a pure crystalline substance is zero at absolute zero
A.
OB AS = grev/T at constant temperature
for any spontaneous process, the entropy of the universe increases
OC.
the entropy of the universe is always constant
AE = q +w

Expert Solution

This question has been solved!

Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.

This is a popular solution!

SEE SOLUTION Check out a sample Q&A here

Step 1

VIEW

Step 2

VIEW

Final answer

VIEW

Trending now

This is a popular solution!

Step by step

Solved in 3 steps

SEE SOLUTION Check out a sample Q&A here

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

For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
The synthesis of glucose directly from CO2 and H2O and the synthesis of proteins directly from amino acids are both non-spontaneous processes under standard conditions. Yet it is necessary for these to occur for life to exist. In light of the second law of thermodynamics, how can life exist?
What is the second law of thermodynamics? For any process, there are four possible sign combinations for Ssys and Ssurr. Which sign combination(s) always give a spontaneous process? Which sign combination(s) always give a non-spontaneous process? Which sign combination(s) may or may not give a spontaneous process?
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the formation of hydrogen sulfide from the elements? H2(g)+18S8(s)H2S(g)
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)
Under what conditions is the entropy of a substance equal to zero?
The standard molar entropy of methanol vapor, CH3OH(g), is 239.8 J K1 mol-1. (a) Calculate the entropy change for the vaporization of 1 mol methanol (use data from Table 16.1 or Appendix J). (b) Calculate the enthalpy of vaporization of methanol, assuming that rS doesnt depend on temperature and taking the boiling point of methanol to be 64.6C.
Use data from Appendix D to calculate the standardentropy change at 25°C for the reaction CH3COOH(g)+NH3(g)CH3NH2(g)+CO2(g)+H2(g) Suppose that 1.00 mol each of solid acetamide, CH3CONH2(s), and water, H2O(l), react to give thesame products. Will the standard entropy change belarger or smaller than that calculated for the reactionin part (a)?
Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
The third law of thermodynamics states that the entropy of a perfect crystal at 0 K is zero. In Appendix 4, F(aq), OH(aq), and S2(aq) all have negative standard entropy values. How can S values be less than zero?