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 O AS = 0 The water condenses to a liquid at a constant temperature of 3.0 °C. A few grams of water vapor (H,O). O As>0 not enough information O As< 0 The carbon dioxide is cooled from O As = 0 62.0 °C to -1.0 °C and is also A few moles of carbon dioxide (CO,) gas. expanded from a volume of 3.0 L to O As> 0 a volume of 4.0 L. not enough information O AS< 0 The helium is cooled from 26.0 °C to O AS = 0 A few moles of helium (He) gas. -13.0 °C while the volume is held O AS> 0 constant at 2.0 L. not enough information

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 O AS = 0 The water condenses to a liquid at a constant temperature of 3.0 °C. A few grams of water vapor (H,O). O As>0 not enough information O As< 0 The carbon dioxide is cooled from O As = 0 62.0 °C to -1.0 °C and is also A few moles of carbon dioxide (CO,) gas. expanded from a volume of 3.0 L to O As> 0 a volume of 4.0 L. not enough information O AS< 0 The helium is cooled from 26.0 °C to O AS = 0 A few moles of helium (He) gas. -13.0 °C while the volume is held O AS> 0 constant at 2.0 L. not enough information

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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Consider the following reaction. Use the information here to determine the value of ΔSsurr at 355 K. Predict whether or not this reaction will be spontaneous at this temperature.2NO(g) + O2(g) -----> 2NO2(g) ΔH = -114 kJ Group of answer choices ΔSsurr = +114 kJ/K, reaction is not spontaneous ΔSsurr = -321 J/K, reaction is not spontaneous ΔSsurr = +114 kJ/K, reaction is spontaneous ΔSsurr = +321 J/K, reaction is spontaneous ΔSsurr = +321 J/K, it is not possible to predict the spontaneity of this reaction without more information.
Entropy is the randomness of a system. At the molecular level, entropy can be described in terms of the possible number of different arrangements of particle positions and energies, called microstates. The more microstates the system has, the greater its entropy. Another way of looking at entropy is that the universe is moving toward a broader distribution entropy has since been constantly increasing by distributing this energy. Heat distribution from high temperature to low temperature is a another example of this phenomenon. energy. The universe has a constant amount of energy as stated in the first law of thermodynamics. The universe started with low entropy (concentrated in the moment before the "big bang") and the Part A Rank these systems in order of decreasing entropy. Rank from highest to lowest entropy. To rank items as equivalent, overlap them. > View Available Hint(s) Reset Help Greatest entropy Least entropy 1 mol of helium gas at 273 K and 20L 1 mol of 1 mol of helium gas…
Read the descriptions of physical or chemical changes in the table below. Then decide whether the change will be spontaneous, if you can. Change An exothermic chemical reaction between a solid and a liquid results in gaseous products. A solid precipitates from a solution, absorbing heat as it does so. A gas expands, absorbing heat from its surroundings. Is this change spontaneous? Yes. No. Can't decide with information given. Yes. No. O Can't decide with information given. Yes. No. Can't decide with information given. X
Calculate the change of the entropy of the system in J/K for the following phase transition: condensation of 64.1 g methanol The molar mass of methanol (CH3OH) is 32.04 g/mo%; the enthalpy of vaporization of methanol is 37.6 kJ/mol; the boiling point of methanol is 64.7°C A) -3640 B) -1130 C) 1.13446677 D) -223 E) 0.22258
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…
Calculate ΔS when 25.0 g ethanol at 50.0 °C is added to 75.0 g ethanol at 10.0 °C in an insulated container where Cp = 111.5 J/mol K. Calculate the change in entropy of each ethanol sample, and then the total entropy change. Comment on what is happening to each sample, and overall. (answers: warm = -6.11 J/K; cold = +5.69 J/K; total = 0.42 J/K)
The change in entropy, ΔSrxn∘, is related to the change in the number of moles of gas molecules, Δngas. Determine the change in the moles of gas for each of the reactions and decide if the entropy increases, decreases, or has little or no change. A. C(s)+H2O(g) ⟶ CO(g)+H2(g) Δ?gas= ? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases B. H2O2(l) ⟶ H2(g)+O2(g) Δ?gas=? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases C. C2H2(g)+3O2(g) ⟶ 2CO2(g)+2H2O(l) Δ?gas=? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases D. PCl5(s) ⟶ PCl3(l)+Cl2(g) Δ?gas=? The entropy, ΔSrxn∘, 1) has little or no change 2) increases 3) decreases
3. What change will increase the entropy of the system? Group of answer choices liquid to solid solid to gas gas to liquid gas to solid 2.ΔSsyst>0 for the following reaction: Group of answer choices A, 2NO (g) + O2(g) → 2NO2(g) B, HCl (g) + NH3(g) → NH4Cl (s) C, C3H8(g) + 5 O2(g) → 3CO2 (g) + 4 H2O (g) D, 2N2 (g) + 3H2(g) → 2NH3(g) E, Pb2+(aq) + 2Cl-(aq) → PbCl2 (s)
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
Which of the following describes the second law of thermodynamics?deltaS(system) + deltaS (surroundings) <0deltaS (system) - deltaS (surroundings) = 0deltaS(system) - deltaS (surroundings) <0deltaS(system) - deltaS (surroundings) > 0deltaS(system) + deltaS (surroundings) = 0deltaS (system) + deltaS (surroundings) > 0
Calculate the change in entropy that occurs in the system when 1.10 mol of isopropyl alcohol (C3H§O) melts at its melting point (– 89.5 °C). AH = 5.37 kJ/mol. fus Express your answer in joules per kelvin to three significant figures.
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 liquid acetone ((CH₂)₂CO). A few moles of carbon dioxide (CO₂) gas. A few moles of helium (He) gas. Change The acetone is cooled from 78.0 °C to 9.0 °C. The carbon dioxide is heated from -15.0 °C to 46.0 °C and also expands from a volume of 7.0 L to a volume of 14.0 L. The helium is cooled from 70.0 °C to 8.0 °C while the volume is held constant at 11.0 L. AS O AS 0 O AS 0 not enough information O not enough information O O AS 0 not enough information 5