For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy Sof the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column.SystemChangeASAS < 0The helium is cooled from 66.0 °C toAS = 0A few moles of helium (He) gas.2.0 °C and is also compressed from avolume of 15.0 L to a volume ofAS > 05.0 L.not enoughinformationoloAS < 0ArAS = 0The acetone is cooled from 33.0 °CA few grams of liquid acetone ((CH3)2CO).to 2.0 °C.AS > 0not enoughinformationAS < 0AS = 0The helium expands from a volumeof 5.0 L to a volume of 7.0 L whilethe temperature is held constant atA few moles of helium (He) gas.AS > 07.0 °C.not enoughinformationO O

By cooling ( decreasing the temperature ) we decrease the randomness or entropy of the system, So…

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change AS

For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change AS

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

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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For eac em listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few grams of liquid ammonia (NH3). A few moles of helium (He) gas. Change The carbon dioxide is cooled from 73.0 °C to 8.0 °C while the volume is held constant at 8.0 L. The ammonia evaporates at a constant temperature of 53.0 °C. The helium is cooled from 66.0 °C to 8.0 °C and is also compressed from a volume of 13.0 L to a volume of 10.0 L. ΔS AS 0 not enough information AS 0 not enough information AS 0 not enough information ( [U::: OL E
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S , or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change S A few moles of carbon dioxide (CO2) gas. The carbon dioxide is heated from 9.0 °C to 36.0 °C and also expands from a volume of 6.0 L to a volume of 14.0 L. <S0 =S0 >S0 not enough information A few moles of helium (He) gas. The helium expands from a volume of 9.0 L to a volume of 15.0 L while the temperature is held constant at 20.0 °C. <S0 =S0 >S0 not enough information A few grams of liquid ammonia (NH3). The ammonia is heated from -1.0 °C to 2.0 °C. <S0…
For each of the following changes, do you expect the entropy to increase or decrease? (These questions do not require calculations.) a. Ammonia gas and hydrogen chloride gas react to deposit solid ammonium chloride on a surface b. Two aqueous solutions are combined to form a precipitate c. Methanol gas condenses to form liquid methanol d. Butane liquid reacts with oxygen gas to form carbon dioxide gas and gaseous water e. Liquid water freezes to form ice f. Solid lead melts g. A solid solute dissolves in a liquid solvent h. Liquid water boils Possible answers: 1. Entropy should increase (more positive) 2. Entropy should decrease (more negative) 3. The change in entropy cannot be determined from the information given
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few grams of ammonia vapor (NH3). A few moles of nitrogen (N₂) gas. A few moles of nitrogen (N₂) gas. Change The ammonia condenses to a liquid at a constant temperature of -8.0 °C. The nitrogen is cooled from 78.0 °C to 3.0 °C while the volume is held constant at 2.0 L. The nitrogen is heated from -16.0 °C to 12.0 °C and also expands from a volume of 1.0 L to a volume of 10.0 L. AS AS 0 not enough information AS 0 O not enough information O AS 0 not enough information Ś
Which of the following is true ? X. Exothermic reactions are spontaneous because formation of products is favored by decrease of free energy of the system Y. All spontaneous reactions accompanied by increase of entropy of the universum. Z. All spontaneous reactions accompanied by increase of entropy of the system. * Y only * X, Y and Z * Y and Z only * X only * X and Z only * Z only * X and Y only * none of them
A Moving to another question will save this response. Question 11 A reaction has an equilibrium constant (K) of 58.2. If the entropy of this reaction is-36.7 J/mol"K at a temperature of 317 K, what is the enthalpy of this reaction in kJ/mol? Report your answer to one decimal place. If your answer is negative, make sure to input a negative sign (-). Moving to another question wvill save this response. lyp 144 &
Which of the givenn processes will cause a decrease in entropy? Note only one is correct. - dissolving NaCl in water? - removing a partition to mix two gases? - freezing water to make ice? - boiling water to make steam? - heating ice to make water?
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For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System A few moles of carbon dioxide (CO₂) gas. A few grams of liquid ammonia (NH3). A few moles of carbon dioxide (CO₂) gas. Change The carbon dioxide expands from a volume of 10.0 L to a volume of 13.0 L while the temperature is held constant at 57.0 °C. The ammonia evaporates at a constant temperature of 11.0 °C. The carbon dioxide is cooled from 87.0 °C to -2.0 °C and is also expanded from a volume of 8.0 L to a volume of 11.0 L. AS AS 0 not enough information AS 0 not enough information AS 0 not enough information
At 0.9 bar of pressure and 373.15 K, the hypothetical transition from liquid to gaseous water will result in what change in the total entropy of the “universe”? No change An increase in the total entropy A decrease in the total entropy Not enough information to determine
For each system listed in the first column of the table below, decide (if possible) whether the change described in the second column will increase the entropy S of the system, decrease S, or leave S unchanged. If you don't have enough information to decide, check the "not enough information" button in the last column. System Change AS O AS 0 not enough information O AS 0 not enough O information O AS 0 not enough O information Explanation Check O 2022 McGraw Hill LLC. All Rights Reserved. Terms of Use I Privacy Center | O O
What of the following options describes the term "entropy, S"? O a. If a process or reaction is carried out in multiple steps, the sum of the enthalpy changes for these steps is the same as the enthalpy change if the entire reaction was carried out in a single step. O b. An indication that a process is capable of proceeding in a given direction without needing to be driven by an outside source of energy. O c. A thermodynamic function which measures the dispersal of energy amongst the particles in a substance. O d. The substances or material being studied in an experiment. For a chemical reaction, the system is all of the atoms in the substances undergoing the reaction. O e. Everything outside of the system.