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 Sof 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.Note for advanced students: you may assume ideal gas and ideal solution behaviour.SystemChangeASAS < 0The seawater is passed through areverse-osmosis filter, whichAS = 0A liter of seawater at 15°C.separates it into 750. mL ofpureAS > 0water and 250. mL of brine (verysalty water).not enoughinformationAS < 020. L of pure oxygen (O,) gas andAS = 0The gases are mixed, with the20.0 L of pure hydrogen (H2) gas,pressure kept constant at 2 atm.AS > 0both at 2 atm and – 1°C.not enoughinformationAS < 0300 mL of a solution made from0.5 g of NH,Cl crystallizes out ofAS = 04ammonium chloride (NH,CI)the solution, without changing thetemperature.AS > 0dissolved in water.not enoughinformation

Entropy is defined as the degree of randomness, as it increases entropy also increases.

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.

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.

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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A system of 8,872 particles initially has 3.21*1042 possible configurations. If we remove some of the particles and are left with 3,049 particles in the system what is the change in entropy? You can assume fromthis question the number of possible configurations does not change.Please express answer in scientific notation to the second decimal place
7. For OH-(aq), Sº is -10.7 J/mol-K, which is negative. Which comment below is correct? The hydroxide ion must be perfectly symmetrical and tightly organized. Sº is a relative value: This is an artifact since absolute entropy can't be negative. This must be a mistake since there can't exist fewer than no possibilities. The hydroxide ion is an unusual ion compared with all other aqueous ions.
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 moles of carbon dioxide (CO₂) gas. A few grams of liquid water (H₂O). Change The carbon dioxide expands from a volume of 1.0 L to a volume of 3.0 L while the temperature is held constant at 82.0 °C. The carbon dioxide is cooled from 77.0 °C to 8.0 °C and is also expanded from a volume of 2.0 L to a volume of 12.0 L. The water is heated from -12.0 °C to 63.0 °C. оо O ооо OO AS AS 0 not enough information AS 0 not enough information AS 0 not enough information
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Choose the correct answer out of the three options: Suppose an isolated system undergoes a change and the result is that parts of the system become more disordered. It could be said that such a process (increases/decreases/does not change) the entropy of the system. The entropy change of the system is considered to be (positive/negative/zero).
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 not enough information AS 0 not enough information AS 0 8.0 L. not enough information
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.
Q7. For each reaction, predict the sign of entropy of system and find the value of ASuniv. a. 3NO (g) N₂O (g) + NO2 (g) b. P4 (g) +5 Oz (g) → P4010 (S) c. Combustion of ethane (C2H6) gas to form carbon dioxide and gaseous water.
O ENTROPY AND FREE ENERGY Predicting qualitatively how entropy changes with temperature. OD 15 Nerbs 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 AS O AS 0 not enough O information AS 0 not enough information O AS 0 not enough information Fxplanation Check 0 Terms of Use I Privacy Center| Accessibility O 2022 McGraw Hill LLC. All Rights Reserved. re to search 99+ IA
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
1. Ammonia can be made from the reaction of nitrogen and hydrogen: N2 (g) + 3 H2 (g) ⟺ 2 NH3 (g) For this reaction, K = 1.6 x 102 and ΔH = -91.8 kcal/mole at 25oC. Is the reaction endothermic or exothermic? Briefly explain. Is there in increase in entropy, a decrease in entropy, or no change in entropy? Briefly explain. At 25oC, is this reaction product favored or reactant favored? Briefly explain. Do you expect this reaction to be spontaneous at all temperatures? Briefly explain.