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 The seawater is passed through a reverse-osmosis filter, which AS = 0 A liter of seawater at 15°C. separates it into 750. mL of pure AS > 0 water and 250. mL of brine (very salty water). not enough information O AS < 0 20. L of pure argon (Ar) gas and AS = 0 The gases are mixed, with the 20.0 L of pure helium (He) gas, pressure kept constant at 5 atm. O AS > 0 both at 5 atm and 6°C. not enough information O AS < 0 O AS = 0 1.0 g of sodium iodide (Nal) and The sodium iodide is dissolved in the 2.0 L of pure water at 81 °C. water. 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 Change AS AS < 0 The seawater is passed through a reverse-osmosis filter, which AS = 0 A liter of seawater at 15°C. separates it into 750. mL of pure AS > 0 water and 250. mL of brine (very salty water). not enough information O AS < 0 20. L of pure argon (Ar) gas and AS = 0 The gases are mixed, with the 20.0 L of pure helium (He) gas, pressure kept constant at 5 atm. O AS > 0 both at 5 atm and 6°C. not enough information O AS < 0 O AS = 0 1.0 g of sodium iodide (Nal) and The sodium iodide is dissolved in the 2.0 L of pure water at 81 °C. water. AS > 0 not enough information

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 reaction vessel was filled with H2, CO2, CO, and Molar H2O and the following reaction occurred. Species Entropy H2(g) + CO2(g) = CO(g) + H20(g) The standard state Gibbs free energy change (AG) was (J/mol K) found to be 25.6 kJ/mole at 298K. H2(g) 130.7 CO2(g) a. Calculate the standard state entropy change (AS°) for this reaction. 213.8 CO(g) 197.7 H20(g) 188.8 b. Calculate the standard state enthalpy (AH°) for the reaction at 298K? Note: if you did not find a value for part A use AS° = 65.6 J/molK. c. Given standard state concentrations, at what temperature will the reaction become spontaneous? Note: if you did not find a value for part A use AH° = 31.0 kj/mol.
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. olb Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O As 0 25° C. not enough information O As 0 62°C. not enough information O AS 0 dissolved in water. 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 AS 0 water and 250. mL of brine (very salty water). not enough information AS 0 both at 3 atm and 7°C. not enough information AS 0 at 38 °C. 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 1.0 g of sodium iodide (Nal) and 2.0 L of pure water at 46 °C. Alter of seawater at 15°C. A mixture of hydrogen (H₂) gas and xenon (Xe) gas at 1 atm and 35°C. Change The sodium iodide is dissolved in the water. 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). An additional 2.0 1. of pure Xe gas is added to the mixture, with the pressure kept constant at 1 atm. AS O AS 0 hot enough information
4.00 L of ar and 2.50 L of he, each at 298 K and 1.50 atm, were mixed isothermally and isobarically. The mixture was then expanded to a final volume of 20.0 L at 298 K. Write chemical processes for each step, and determine the change in entropy for the complete process.
0 i not enough information AS 0 not enough information O AS > 0 AS = 0 Edit not enough information 17 ●●● €
Identify whether there will be an increase or a decrease in entropy for the system. Nitrogen gas reacts with hydrogen gas to produce ammonia gas. N2(g) + 3H2(g) → 2 NH3(g) the condensation of steam dry ice subliming magnesium solid reacting with molecular oxygen to produce solid magnesium oxide. 2 Mg(s) + O2(g) → 2 MgO(s)
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. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System A liter of seawater at 15° C. A mixture of xenon (Xe) gas and nitrogen (N₂) gas at 1 atm and 22° C. 1.0 g of potassium iodide (KI) and 2.0 L of pure water at 42 °C. Change 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). An additional 2.0 L of pure N₂ gas is added to the mixture, with the pressure kept constant at 1 atm. The potassium iodide is dissolved in the water. O O AS AS 0 not enough information AS 0 not enough information AS 0 not enough information
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. Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS AS 0 not enough information AS 0 3°C. not enough information AS 0 both at 37.°C. flows through the bag into the sucrose solution. not enough information O O
Predicting qualitatively how entropy changes with temperature and volume 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 acetone vapor ((CH₂)₂CO). A few moles of helium (He) gas. A few moles of helium (He) gas. Predicting qualit Change The acetone condenses to a liquid at a constant temperature of -12.0 °C. The helium is heated from -19.0 °C to 59.0 °C while the volume is held constant at 10.0 L. The helium is heated from 0.0 °C to 3.0 °C and is also compressed from a volume of 13.0 L to a volume of 10.0 L. tion ΔS O AS 0 O not enough information Ο ΔS 0 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 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
I took out an ice cube from the -10°C freezer and wanted to add it to the drink, but was immediately called away and forgot to add it to the drink. When I came back, I saw that the ice cube had completely melted into water at a room temperature of 25°C. Assuming that the ice cube is exactly 2 mole, and regard this ice cube as a system, try to calculate the change of enthalpy and entropy (△H,△S) of the system. Let the heat capacity of water be 25 JK-1mol-1, the heat capacity of ice be 15 JK-1mol-1 and the heat of melting of ice △Ĥfus = 6 kJ/mol.