Which statements are true about entropy? More than one statement may be correct. The molar entropy of a substance at any temperature can be determine exactly. The absolute entropy of a substance between OK and 15 K cannot be calculated exactly. |If it were possible to produce a perfect crystalline element with a temperature of absolute zero, then absolute entropy of this substance would be zero. The third law of thermodynamics has been found to be consistent with experimental observations for temperatures approaching zero Kelvin.

Which statements are true about entropy? More than one statement may be correct. The molar entropy of a substance at any temperature can be determine exactly. The absolute entropy of a substance between OK and 15 K cannot be calculated exactly. |If it were possible to produce a perfect crystalline element with a temperature of absolute zero, then absolute entropy of this substance would be zero. The third law of thermodynamics has been found to be consistent with experimental observations for temperatures approaching zero Kelvin.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section16.3: Measuring Dispersal Of Energy: Entropy

Problem 16.3CE

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Under what conditions is the entropy of a substance equal to zero?
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)?
In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?
The third law of thermodynamics says that a perfect crystal at 0 K has zero entropy. The standard entropy of a substance, S can be determined by evaluating the energy required to carry out conversion from 0 K to standard conditions. What information would be needed to calculate S for liquid water at 298 K and 1 bar?
The standard molar entropy of iodine vapor, I2(g), is 260.7 J Kl mol-1 and the standard molar enthalpy of formation is 62.4 kJ/mol. a) Calculate the entropy change for vaporization of 1 mol of solid iodine (use data from Table 16.1 or Appendix J). b) Calculate the enthalpy change for sublimation of iodine. c) Assuming that rSdoes not change with temperature, estimate the temperature at which iodine would sublime (change directly from solid to gas).
Explain why the statement No process is 100 efficient is not the best statement of the second law of thermodynamics.
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.
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?
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Explain why absolute entropies can be measured.