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.SystemChangeASO AS < 0300 mL of a solution made fromO AS = 0potassium bromide (KBr) dissolvedin water.0.5 g of KBr crystallizes out of thesolution, without changing thetemperature.O AS > 0not enoughinformationO AS < 0A solution made of potassiumO AS = 050. mL of pure water is added tobromide (KBr) in water, at 15°C.the solution.O AS > 0not enoughinformationO AS < 0A mixture of oxygen (O,) gas andO AS = 0An additional 2.0 L of pure Kr gasis added to the mixture, with thekrypton (Kr) gas at 3 atm and- 12°C.O AS > 0pressure kept constant at 3 atm.not enoughinformation

Entropy, the measure of a system's thermal energy per unit temperature that is unavailable for doing useful work. Entropy is also a measure of the molecular disorder, or randomness, of a system.(a) In the first case, the KBr is dissolved to form a solution and then crystallizes out of the solution. There is no change in temperature. The aqueous state is converted to a solid-state which decreases the randomness of the substance. Therefore, the entropy of the system decreases. ΔS < 0. (b) In this case, there is a change in the volume of the solution. An increase in volume results in a decrease in concentration. Therefore, the entropy of a system increases as the concentrations of the components decrease. Changes in volume will lead to changes in entropy. The larger the volume the more ways there are to distribute the molecules in that volume; the more ways there are to distribute the molecules (energy), the higher the entropy. An increase in volume will increase entropy. ΔS > 0 (c) Addition of inert gas at constant pressure. In this case, the total volume will increase. Hence, the number of moles per unit volume will decrease. The larger the volume the more ways there are to distribute the molecules in that volume; the more ways there are to distribute the molecules (energy), the higher the entropy. An increase in volume will increase entropy. ΔS > 0

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Chemistry

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 Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS < 0 300 mL of a solution made from O AS = 0 0.5 g of KBr crystallizes out of the solution, without changing the temperature. potassium bromide (KBr) dissolved O AS > 0 in water. not enough information O AS < 0 O AS = 0 A solution made of potassium bromide (KBr) in water, at 15°C. 50. mL of pure water is added to the solution. O AS > 0 not enough information O AS < 0 A mixture of oxygen (O,) gas and O AS = 0 An additional 2.0 L of pure Kr gas is added to the mixture, with the krypton (Kr) gas at 3 atm and - 12°C. O AS > 0 pressure kept constant at 3 atm. not enough

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 Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS < 0 300 mL of a solution made from O AS = 0 0.5 g of KBr crystallizes out of the solution, without changing the temperature. potassium bromide (KBr) dissolved O AS > 0 in water. not enough information O AS < 0 O AS = 0 A solution made of potassium bromide (KBr) in water, at 15°C. 50. mL of pure water is added to the solution. O AS > 0 not enough information O AS < 0 A mixture of oxygen (O,) gas and O AS = 0 An additional 2.0 L of pure Kr gas is added to the mixture, with the krypton (Kr) gas at 3 atm and - 12°C. O AS > 0 pressure kept constant at 3 atm. not enough

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 each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS, If it's not Ixn" possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction sign of reaction entropy AS 0 AS rxn not enough information. AS 0 AS rxn not enough information. AS 0 not enough information. ?
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. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System A mixture of oxygen (O₂) gas and hydrogen (H₂) gas at 3 atm and 7°C. A liter of seawater at 15°C. 300 mL of a solution made from sodium iodide (Nal) dissolved in water. Change An additional 2.0 L of pure H₂ gas is added to the mixture, with the pressure kept constant at 3 atm. The seawater is passed through a reverse-osmosis filter, which separates it into 750. mL of pure water and 250. mL of brine (very salty water). 0.5 g of Nal crystallizes out of the solution, without changing the temperature. O O AS 0 O As AS 0 not enough information O not enough. information O AS 0 not enough…
Please don't provide handwritten solution ....
Let's say that when you perform the Entropy of Dissolution of Urea Lab that you calculate the values listed below. Using those values, calculate the entropy change for the system. ΔH=12.5kJ; ΔG=−5.26kJ; Temperature of Surroundings=22.00C Group of answer choices +24.5 J/mole-Kelvin +32.9 J/mole-Kelvin +60.2 J/mole-Kelvin +277 J/mole-Kelvin
a) With reference to the molecules below, explain the factors which govern the watersolubility and melting points and explain the differences in the values observedbelow.b) You are a chemical engineer working in a pharmaceutical manufacturing plant.You’ve been tasked with scaling up the synthesis of a potential drug candidate.From previous studies, you know the following information about reaction takingplace:ΔHoreaction = -112.2kJΔS = -15.26JK-1mol-1ΔG = -18.81kJ Discuss the meaning of each term/value and what this tells you aboutthe nature of the reaction. Given the above information, briefly state the impact of low/hightemperatures on the above reaction.
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es) Qualitatively predicting reaction entropy For each chemical reaction listed in the first column of the table below, predict the sign (positive or negative) of the reaction entropy AS If it's not possible to decide with the information given, check the "not enough information" button in the last column. Note for advanced students: Assume the temperature remains constant. Assume all gases and solutions are ideal. reaction N₂(g) + 3H₂(g) → 2NH, (e) 4Fe()+30.)- 2Fe₂O, (s) N. (3), (g) 2NH, (g) sign of reaction entropy 04 ron reaction <<0 50 not enough information. 45x 250 <<0 not enough information. 450 50 not enough information. Using the general properties of Gibbs free energy The standard reaction free energy AG" --835. kJ for this reaction: 2 Al(s) + Fe₂O3(s)-Al₂O3(s) + 2 Fe(s) Use this information to complete the table below. Round each of your answers to the nearest kJ. BALAKEN F04 AGO Focus
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. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS AS 0 not enough information AS 0 both at 37.°C. flows through the bag into the sucrose solution. not enough information AS 0 and 22°C. pressure kept constant at 2 atm. not enough information
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. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS CO A solution made of ammonium bromide (NH Br) in water, at O AS = 0 50. mL of pure water is added to the solution. O AS >0 27°C. not enough information O AS 0 t 27 °C. not enough information O AS 0 argon (Ar) gas at 2 atm and 8°C. pressure kept constant at 2 atm. not enough information
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