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 helium (He) gas. A few moles of nitrogen (N₂) gas. A few moles of helium (He) gas. Change The helium is cooled from 25.0 °C to -2.0 °C while the volume is held constant at 11.0 L. The nitrogen is cooled from 83.0 °C to -12.0 °C and is also expanded from a volume of 7.0 L to a volume of 13.0 L. The helium is compressed from a volume of 12.0 L to a volume of 8.0 L while the temperature is held constant at -1.0 °C. X O O O O AS AS < 0 AS = 0 OO AS > 0 not enough information Ο ΔS < 0 O AS = 0 O AS > 0 not enough information O AS < 0 O AS=0 Ο ΔS > 0 AS not enough O information Ś

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 helium (He) gas. A few moles of nitrogen (N₂) gas. A few moles of helium (He) gas. Change The helium is cooled from 25.0 °C to -2.0 °C while the volume is held constant at 11.0 L. The nitrogen is cooled from 83.0 °C to -12.0 °C and is also expanded from a volume of 7.0 L to a volume of 13.0 L. The helium is compressed from a volume of 12.0 L to a volume of 8.0 L while the temperature is held constant at -1.0 °C. X O O O O AS AS < 0 AS = 0 OO AS > 0 not enough information Ο ΔS < 0 O AS = 0 O AS > 0 not enough information O AS < 0 O AS=0 Ο ΔS > 0 AS not enough O information Ś

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
Which of the following result in an increase in the entropy of the system? I. H-H II. Br₂(g) → Br₂(7) III. NaBr(s) — Na*(aq) + Br (aq) IV. 02(298 K) → O₂(373 K) V. NH3(1 atm, 298 K) → NH3(3 atm, 298 K) I II, V I, III, IV I, II, III, IV I, II, III, V
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
1:44 1 LTE 4 1 Search Question 20.b of 23 Show Answer Consider the reaction Cl2(g) + Br2(g) → 2 BrCI(g) at 25 °C. Which of the following best explains why the change in entropy is so small? A) All of the components in the chemical equation are gases. B) There are the same moles of gas on both sides of the reaction. C) The temperature of the reaction does not change. Tap here or pull up for additional resources
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
3) Place the following in order of increasing molar entropy at 298 K. a) CO2 C3H8 SO b) NaCl(s) Na3PO4(aq) NaCl(aq)
chapter 12: 13) Chlorofluorocarbons (CFCs) are no longer used as refrigerants because they help destroy the ozone layer. Trichlorofluoromethane (CCl3F) boils at 23.8°C, and its molar heat of vaporization is 24.8 kJ/mol. Calculate the molar entropy of evaporation of CCl3F(ℓ).
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
Which one of the following choices of gaseous molecules is rank ordered correctly from lowest standard molar entropy (left hand side) to highest standard molar entropy (right hand side)? He, Ne, CO, SiH4 SiH4 , CO, Ne, He SiH4 , Ne, CO, He CO, SiH4 , Ne, He
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.