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 entro 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 col Note for advanced students: you may assume ideal gas and ideal solution behaviour. System A solution made of sodium bromide (NaBr) in water, at 24°C. A 0.35M solution of sucrose in water, and a beaker of pure water, both at 37. C 20. L of pure nitrogen (N₂) gas and 20.0 L of pure krypton (Kr) gas, both at 5 atm and -11°C Change 50. ml. of pure water is added to the solution. The solution is put into a semipermeable bag immersed in the water, and 50. ml. of pure water flows through the bag into the sucrose solution. The gases are mixed, with the pressure kept constant at 5 atm AS O AS <0 0 AS-0 O AS > 0 O not enough information O AS <0 045-0 O AS > 0 O not enough information O AS CO O AS-0 O AS > 0 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 entro 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 col Note for advanced students: you may assume ideal gas and ideal solution behaviour. System A solution made of sodium bromide (NaBr) in water, at 24°C. A 0.35M solution of sucrose in water, and a beaker of pure water, both at 37. C 20. L of pure nitrogen (N₂) gas and 20.0 L of pure krypton (Kr) gas, both at 5 atm and -11°C Change 50. ml. of pure water is added to the solution. The solution is put into a semipermeable bag immersed in the water, and 50. ml. of pure water flows through the bag into the sucrose solution. The gases are mixed, with the pressure kept constant at 5 atm AS O AS <0 0 AS-0 O AS > 0 O not enough information O AS <0 045-0 O AS > 0 O not enough information O AS CO O AS-0 O AS > 0 not enough

Chemistry: An Atoms First Approach

2nd Edition

ISBN:9781305079243

Author:Steven S. Zumdahl, Susan A. Zumdahl

Publisher:Steven S. Zumdahl, Susan A. Zumdahl

Chapter16: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 114CP: Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution...

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Carbon tetrachloride (CCl4) and benzene (C6H6) form ideal solutions. Consider an equimolar solution of CCl4 and C6H6 at 25C. The vapor above the solution is collected and condensed. Using the following data, determine the composition in mole fraction of the condensed vapor. Substance Gfo C6H6(l) 124.50 kJ/mol C6H6(g) 129.66 kJ/mol CCI4(l) 65.21 kJ/mol CCI4,(g) 60.59 kJ/mol
Two students prepared aqueous solutions of LiCl and measured the properties, as shown in the table above. Both students observed that the solid LiCl readily dissolved in H2O. The students drew particle diagrams to explain the changes in the enthalpy and entropy of dissolution for LiCl based on their results and observations. Based on this information, the better particle diagram was drawn by which student, and why is that diagram more accurate? (see attached image) a.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+ and Cl− ions causing an increase in entropy. b.) The better particle diagram was drawn by Student 1 because when LiCl dissolves in water, it dissociates into Li+and Cl−ions indicating that the dissolution of LiCl is exothermic. c.) The better particle diagram was drawn by Student 2 because it shows that LiCl does not dissociate, resulting in a decrease in entropy for the dissolution of LiCl.…
1/5 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 not enough information O AS 0 and 34°C. pressure kept constant at 4 atm. not enough O. information O AS 0 dissolved in water. not enough information Enplanation Check Terms of Use | Privacy Center | Accessibilit 02022 McGraw Hill LLC. All Rights Reserved. DE O O O O O
Derive an effective Henry’s constant formula for ammonia (NH3) dissolved in water
When NaCl(s) is dissolved in a mixture of ice and liquid water, all originally at 0oC, the temperature of the mixture drop. Which does NOT occur in this process? A)Some of the ice melt; B)Heatflow from the liquid (solution) to the solid (ice); C)The freezing point of the solution is lowered; D)The chemical potential of the liquid water increases; E)The entropy of the Universe is decreasing.
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 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 xenon (Xe) gas and hydrogen (H₂) gas at 2 atm and 48°C. 300 mL of a solution made from ammonium iodide (NH4I) dissolved in water. A solution made of ammonium iodide (NH I) in water, at 58°C. Change An additional 2.0 L of pure H₂ gas is added to the mixture, with the pressure kept constant at 2 atm. 0.5 g of NH I crystallizes out of the solution, without changing the temperature. 50. mL of pure water is added to the solution. AS ⒸAS 0 not enough information AS 0 not enough information AS 0 not enough information ? 00. 18 Ar BA Ò
Hexane and heptane are miscible with eachother in all proportions. In making a solution of them, isthe entropy of the system increased, decreased, or close tozero, compared to the separate pure liquids?
6. For the given data draw graph Hydrogen monochloride (HCI) Solubility Potassium Chloride (KCI) Solubility Temperature Solubility (g of HCI /100 mL of H20) (°C) Temperature Solubility (g of KCI /100 mL of H20) (°C) 85 27 10 78 10 30 20 71 20 33 30 66 30 36 40 62 40 39 60 55 60 46 80 49 80 52 100 42 100 58
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 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 colum Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 both at 37.°C. not enough O information O AS 0 water and 250. mL of brine (very not enough information salty water). O AS 0 pressure kept constant at 2 atm both at 2 atm and 22°C. not enough information Explanation Check 02022 McGraw Hill LLC. All Rights Reserved. Terms of Use | Privacy Center | Accessi IA 99+ to search
f dissolving 1.5 g of a solute into 100 mL of water caused the temperature of the solution toincrease by 4.7 ⁰C, what would the change of temperature be if 3.0 g of the solute were dissolvedin the same volume of water? Explain.
Consider two ionic solids, both composed of singly-charged ions, that have different lattice energies. Which solid will be more soluble in water, the one with the larger lattice energy or the one with the smaller lattice energy? Assume that solute-solvent interactions are the same for both solids. The solid with the smaller lattice energy. The solid with the smaller lattice energy, if entropy increases as a result of mixing and the solid with the larger lattice energy, if entropy decreases as a result of mixing. The solid with the larger lattice energy. They will have the same or very similar solubilities. The solid with the larger lattice energy, if entropy increases as a result of mixing and the solid with the smaller lattice energy, if entropy decreases as a result of mixing.
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 dissolved in water. not enough information AS 0 27° C. not enough information O AS 0 gas, both at 3 atm and -20°C. not enough information