Problem 19.36 - Enhanced - with Feedback Part A Does the entropy of the system increase, decrease, or stay the same for each of the following conditions. Drag the appropriate items to their respective bins. Increases The volume of a gas increases. The temperature of the system increases. Decreases Equal volumes of ethanol and water are mixed to form a solution. Stays the same Reset Help

Problem 19.36 - Enhanced - with Feedback Part A Does the entropy of the system increase, decrease, or stay the same for each of the following conditions. Drag the appropriate items to their respective bins. Increases The volume of a gas increases. The temperature of the system increases. Decreases Equal volumes of ethanol and water are mixed to form a solution. Stays the same Reset Help

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 two separate containers: container A holds 65.3 g of carbon dioxide gas, container B holds 48.2 g of oxygen gas. The pressure of both gases is 1 bar and the temperature is 298.15 K. Both gases can be treated as ideal gases. Parta) Determine the sum of the entropies of the gases in both separated containers. Part b) Calculate the total entropy of the gas mixture, which is obtained after mixing both gases in one container, while maintaining a constant temperature and pressure. Part c) The gas mixture from part b) is expanded in an isobaric process until its volume has increased by a factor of 2.5. Calculate the entropy of the gas mixture after this process is completed.
Answer number 39-48 pls. I don't want to waste my money here.
1. Calculate the number of possible microstates in system (A): one particle and four slots. 2. Calculate the number of possible microstates in system (B): three particles and four slots. 3. 4. Calculate the entropy difference between the two systems (A) and (B). Systems A and B, are combined into system C, shown above. Calculate the total number of microstates when (A) and (B) are merged together to give (C). 5. If two quanta of energy are added to this system, Wotal = Wparticles X Wquanta Energy quanta can pass between the two subsystems, but particles cannot. Energy quanta can only be located on a particle, not in an empty box. You may add as many quanta as you like o any given particle. Calculate the total number of unique energy arrangements W of system C. 6. The barrier between the two parts of system C is removed so that particles can move throughout the combined system. Calculate the total number of unique arrangements Wtotal.
Discuss the diagram of the molar Gibbs free energy (or chemical potential) versus temperaturebelow for a pure substance. Why are there three curves? Why do they slope downward? Does thegraph identify any interesting temperatures? Are some segmentsof the curves more important/interesting than others? Feel free to redraw and label the diagram.
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 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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When a liquid is converted to a solid, entropy increases. OTrue O False
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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