Activity 2: Direction: Predict whether the entropy will increase or decrease for each of the following processes. Briefly state the reason for each answer.Write your answer on a separate sheet of paper. 1. ice cream melts. 2. water vapor deposits as ice crystals on a cold window pane. 3. iodine crystals undergo sublimation. 4. sugar dissolves in a cup of water. 5. water is heated until lukewarm. 6. 2SO2i + Ozi 7. NHa + HCl(g) 8. MGCO30 9. producing ammonia from its elements 10. freezing of water. NH.Cl MgO + COzu

Activity 2: Direction: Predict whether the entropy will increase or decrease for each of the following processes. Briefly state the reason for each answer.Write your answer on a separate sheet of paper. 1. ice cream melts. 2. water vapor deposits as ice crystals on a cold window pane. 3. iodine crystals undergo sublimation. 4. sugar dissolves in a cup of water. 5. water is heated until lukewarm. 6. 2SO2i + Ozi 7. NHa + HCl(g) 8. MGCO30 9. producing ammonia from its elements 10. freezing of water. NH.Cl MgO + COzu

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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Which substance has the higher entropy? a. a sample of pure silicon (to be used in a computer chip) or a piece of silicon containing a trace of another element such as boron or phosphorus a piece of silicon containing a trace of another element such as boron or phosphorus a sample of pure silicon b. CO2(g) at 0 °C or CO2 (g) at -50 °C O CO2 (g) at –50 °C O CO2 (g) at 0 °C c. I2 (s) or I2 (g) both at room temperature OL (g) OL (s) d. one mole of CO2(g) at 1 bar pressure or one mole of CO2(g) at 0.01 bar pressure (both at 298 K) one mole of CO2(g) at 0.01 bar pressure one mole of CO2(g) at 1 bar pressure
Which change is likely to be accompanied by an increase in entropy? A. N2 (g) + 3 H2 (g) → 2 NH3 (g) at 25 °C + AgCl (s) at 25 °C B. Ag* (aq) + CF (aq) C. CO2 (s) → CO2 (g) at -70 °C D. H20 (g) = H2O (I) at 100 °C
Which of the following statements is false? a. Entropies of ionic solids that have similar formulas are larger when the attractions among the ions are stronger. b. Entropy usually decreases when a gas is dissolved in a liquid. c. Entropy usually increases when a pure liquid or solid dissolves in a solvent. d. Entropies of more complex molecules are larger than those of simpler molecules. e. Entropies of gases are usually much larger that those of liquids, which in turn are usually larger than those of solids.
choose the right options -When a solid dissolves in a liquid, entropy usually (increases or decreases?) So the value for ΔΔS is (positive or negative?) Remember that negative values of ΔΔG are favorable, and ΔΔG = ΔΔH - TΔΔS. Consequently, solids are usually more soluble at (higher or lower?) temperatures. When a gas dissolves in a liquid, entropy usually (increases or decreases), so the value for ΔΔS is (negative or postive) Remember that negative values of ΔΔG are favorable, and ΔΔG = ΔΔH - TΔΔS. Consequently, gases are usually more soluble at (lower or higher) temperatures.
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
Determine whether the change in entropy increases or decreases.The number 1 serves as an example. increase(L-G) 1. Evaporation 2.Solidification 3.Deposition 4.Fusion 5.Condensation 6.Lowering the temperature of ethyl alcohol from 30° C to 10°.
The answer may be One or more than One options Choose statements that describe ΔStotal ≥ 0. When we say that entropy is constant or unchanging, it may have infinitesimally small fluctuations about its average value. You may want to consult the entropy handout from Week 5. a. During a reversible process, the entropy of any systems is constant. b. The entropy of an isolated system at equilibrium is constant. c. As an isolated system relaxes to an equilibrium state its entropy increases. d. During an irreversible process, the entropy of any system increases. e. During an irreversible process, the entropy of an isolated system decreases. f. During a reversible process, the entropy of an isolated system is constant.
Consider samples of ice, water, and water vapor that all equal in mass. Which of the three samples will have the lowest entropy?
In which of the following processes would the entropy of the system increase? A liquid forming from a gas. A solid forming from a gas. The number of gas molecules increasing during a chemical reaction. A solid precipitating from a solution.
1. In different phases of water, this has the highest entropy because molecules are too farapart to form H-bonds and they can move freely in any direction.
43 44 QUESTION 25 Which of the following involves an increase in the entropy of the system? O Formation a gaseous product from a solid reagent. Condensation of water. Temperature of a solution is lowered. O Formation of a crystal from a supersaturated solution. 4 QUESTION 26 According to the Third Law of Thermodynamics a perfect crystalline substance c have zero entropy at Click Save and Submit to save and submit. Click Save All Answers to save all answers. Search the web ww a S