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 20. L of pure hydrogen (H₂) gas and 20.0 L of pure xenon (Xe) gas, both at 1 atm and -6° C. 300 mL of a solution made from ammonium iodide (NH4I) dissolved in water. A liter of seawater at 15° C. Change The gases are mixed, with the pressure kept constant at 1 atm. 0.5 g of NH I crystallizes out of the solution, without changing the temperature. 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). X ΔS OAS<0 O AS = 0 O AS>0 O not enough information AS <0 O AS = 0 O AS >0 not enough information AS < 0 O AS = 0 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 20. L of pure hydrogen (H₂) gas and 20.0 L of pure xenon (Xe) gas, both at 1 atm and -6° C. 300 mL of a solution made from ammonium iodide (NH4I) dissolved in water. A liter of seawater at 15° C. Change The gases are mixed, with the pressure kept constant at 1 atm. 0.5 g of NH I crystallizes out of the solution, without changing the temperature. 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). X ΔS OAS<0 O AS = 0 O AS>0 O not enough information AS <0 O AS = 0 O AS >0 not enough information AS < 0 O AS = 0 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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ce-SC5 X r19.core.learn.edgenuity.com/player/ Science - SC5181 A 11 12 13 14 15 16 17 18 What is the relationship between the laws of thermodynamics and the 10 percent rule? O As the temperature of a system approaches absolute zero, the amount of entropy approaches zero, which prevents any energy from being lost in the system. Energy cannot be created or destroyed; it can only be transferred or converted from one form to another, so all organisms in a food chain get the same amount of O energy. The universe is a closed system and entropy or disorder will only increase over time, so whenever a transfer of energy occurs, energy is lost in the process. Mark this and return с If two bodies are in thermal equilibrium with a third body that they will also be in equilibrium with each other, so the loss of one organism results in a loss of energy for O all of them. M DELL DO O English O Save and Exit Next O * Submit Oct 6 Kinley Heath x D ⠀ 3:40
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. olo Note for advanced students: you may assume ideal gas and ideal solution behaviour. Ar System Change AS O AS 0 the solution. not enough information O As 0 gas, both at 5 atm and 10°C. not enough information AS 0 both at 37.°C. flows through the bag into the sucrose solution. not enough information
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)
6 please show steps, and explain your steps if you can. thanks!
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 sign of reaction entropy AS 0 rxn not enough information. AS 0 rxn not enough information. AS 0 → rxn 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. System A few moles of carbon dioxide (CO₂) gas. A few grams of liquid ammonia (NH₂). A few moles of carbon dioxide (CO₂) gas. Change The carbon dioxide is cooled from 61.0 °C to -11.0 °C and is also expanded from a volume of 9.0 L to a volume of 14.0 L. The ammonia evaporates at a constant temperature of 54.0 °C. The carbon dioxide expands from a volume of 6.0 L to a volume of 8.0 L while the temperature is held constant at -7.0 °C. X AS O AS 0 O not enough information AS 0 not enough O information O AS 0 not enough information
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. System A few moles of nitrogen (N₂) gas. A few moles of nitrogen (N₂) gas. A few grams of liquid acetone ((CH3)₂CO). Change The nitrogen is cooled from 51.0 °C to -7.0 °C and is also expanded from a volume of 3.0 L to a volume of 14.0 L. The nitrogen expands from a volume of 7.0 L to a volume of 12.0 L while the temperature is held constant at 8.0 °C. The acetone is cooled from 64.0 °C to 5.0 °C. AS AS 0 not enough information AS 0 not enough information AS 0 not enough information Ś
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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 carbon dioxide (CO₂) gas and nitrogen (N₂) gas at 2 atm and -5°C. A 0.35 M solution of sucrose in water, and a beaker of pure water, both at 37. ° C. A solution made of potassium chloride (KC1) in water, at 64°C. Change An additional 2.0 L of pure N₂ gas is added to the mixture, with the pressure kept constant at 2 atm. 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. 50. mL of pure water is added to the solution. AS AS 0 not enough information AS 0 not enough information AS…
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 liquid water (H₂O). A few moles of helium (He) gas. A few moles of carbon dioxide (CO₂) gas. Change The water is cooled from 65.0 °C to -3.0 °C. The helium is heated from -4.0 °C to 69.0 °C while the volume is held constant at 10.0 L. The carbon dioxide is heated from 1.0 °C to 21.0 °C and is also compressed from a volume of 9.0 L to a volume of 6.0 L. AS AS 0 not enough information AS 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 AS 0 both at 3 m and 19°C. not enough information olo AS 0 at 71 °C. not enough information AS 0 water and 250. mL of brine (very salty water). not enough information O O