Part ARank these systems in order of decreasing entropy.Rank from highest to lowest entropy. To rank items as equivalent, overlap them.• View Available Hint(s)ResetHelpGreatest entropyLeast entropy1 mal of1 mol ofcarbon disulfide gas at273 Kand 40 L1 mal ofnitrogan gas at273 K and 40 L1 mol ofxanon gas at1/2 mal of1/2 mol of1/2 mol ofxenon gas atKenan gas atliquid xanonxanon gas at273 K and 40 L273 K and 20 L273 K and 20 L100 K and 20 Lat 100 KO The correct rarking carnot be determined.

Entropy can be defined as the degree of randomness in a system. The lesser the volume, the lesser…

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 mal of xanon gas at 1 mol of carbon disulfide gas at 1 mal of nitrogen gas at 1 mol of xanon gas at 1/2 mal of 1/2 mol of xanon gas at 273 K and 20 L 1/2 mol of liquid xenon at 100 K Kenan gas at 273 K and 4O L 273 K and 40 L 273 K and 40 L 273 K and 20L 100 K and 2D L

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 mal of xanon gas at 1 mol of carbon disulfide gas at 1 mal of nitrogen gas at 1 mol of xanon gas at 1/2 mal of 1/2 mol of xanon gas at 273 K and 20 L 1/2 mol of liquid xenon at 100 K Kenan gas at 273 K and 4O L 273 K and 40 L 273 K and 40 L 273 K and 20L 100 K and 2D L

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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[References) Use the References to access important values if needed for this question. Arrange the following from lowest to highest entropy: CS2 (2), CS2 (g), CCL (g), S(s). Assume 1 mole of each at the same condit from lowest to highest entropy Drag and drop your selection from the following list to complete the answer: CS (g) S(s) CCL (g) CS2 () Submit Answer Try Another Version 2 item attempts remaining
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.
At 363 K, one state is twice as likely as the other. The first (more likely) state has an energy of 9.19 kcal/mol and an entropy of 0.915 kcal/mol-K. The other state has an energy of 2.19 kcal/mol more then the first state. What is the entropy of the second (less likely) state?
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?
Using tabulated values of S°, calculate the standard entropy per mole of atoms for the following. Ar. The S° for Ar is 154.843 J/(mol*K). J*mol1*K1 eTextbook and Media O2. The S° for O2 is 205.152 J/(mol*K). J*mol-1*K*1 O3. The S° for O3 is 238.9 J/(mol*K). J*mol 1*K1 C2H6. The S° for C2H6 is 229.2 J/(mol*K). J*mol 1*K1
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Place the following species in order of decreasing molar entropy at 55°C. Assume that they are all in the gas phase. SiO2 Si4H10 SiO SiO2 > Si4H10 > SiO Si4H10 > SiO2 > SiO SiO2 > SiO > Si4H10 SiO > Si4H10 > SiO2 Si4H10 > SiO > SiO2 SiO > SiO2 > Si4H10
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 carbon dioxide (CO₂) gas. A few moles of carbon dioxide (CO₂) gas. Change The helium is compressed from a volume of 11.0 L to a volume of 4.0 L while the temperature is held constant at -6.0 °C. The carbon dioxide is heated from -17.0 °C to 53.0 °C while the volume is held constant at 8.0 L. The carbon dioxide is heated from -8.0 °C to 3.0 °C and also expands from a volume of 10.0 L to a volume of 12.0 L. x AS AS 0 not enough information O AS 0 not enough information O AS 0 not enough information
Give answer second question with explanation