For each system Risted 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 Sunchanged. 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 ldeal solution behaviour. System Change AS O AS 0 -1"C. o rot enough information O AS0 saty water) not enouh Omation

For each system Risted 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 Sunchanged. 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 ldeal solution behaviour. System Change AS O AS 0 -1"C. o rot enough information O AS0 saty water) not enouh Omation

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter16: Thermodynamics: Directionality Of Chemical Reactions

Section: Chapter Questions

Problem 121QRT

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For the process A(l) A(g), which direction is favored by changes in energy probability? Positional probability? Explain your answers. If you wanted to favor the process as written, would you raise or lower the temperature of the system? Explain.
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
(d) For the reaction: H3C. H3C. C-OH Cc=CH2 H3C H20 H,C H3C Reaction 2 Reaction 2 does not go to completion and the position of the reaction can be defined in terms of the equilibrium constant, K. (i) For the above reaction at 298K under specific conditions the following thermodynamic information were obtained, reaction Gibbs free energy (AreactG = -5.4 kJ mol-1), standard reaction enthalpy (AreactH® = -52.7 kJ mol-1) and standard reaction entropy (AreactS® = -0.16 kJ mol-1). From the above detail, calculate the equilibrium constant. (ii) Sketch a diagram of the Gibbs free energy versus reaction progress and on diagram label the reaction Gibbs free energy (A,react G) and standard reaction Gibbs free energy (Areact G®).
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. ado Note for advanced students: you may assume ideal gas and ideal solution behaviour. System Change AS O AS 0 at 41 °C. not enough information O As 0 and 2° C. pressure kept constant at 2 atm. not enough information O AS 0 water and 250. mL of brine (very salty water). not enough information O O Olo o
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
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
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
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
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 not enough information O AS 0 pressure kept constant at 3 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 0 water. not enough information AS 0 14°C. pressure kept constant at 1 atm. not enough information O AS 0 both at 37.°C. flows through the bag into the sucrose solution. not enough O information ?
entActivity.do?locator-assignment-take Ikanbewy Tfapies Use the References to access important values if needed for this question. Consider the following system at equilibrium where AH° = 10.4 kJ, and K. = 1.80×10 at 698 K: 2HI(g) H2(g) + I½(g) If the TEMPERATURE on the equilibrium system is suddenly increased: The value of K, A. Increases B. Decreases C. Remains the same The value of Q. A. Is greater than K. B. Is equal to K C. Is less than K. The reaction must: A. Run in the forward direction to restablish equilibrium. B. Run in the reverse direction to restablish equilibrium. C. Remain the same. Already at equilibrium. The concentration of I, will: A. Increase. B. Decrease. C. Remain the same. Submit Answer Retry Entire Group 9 more group attempts remaining 50 hp
15. When a solute is able to go spontaneously into solution: (A) both the enthalpy (AHsoln) and the entropy (ASsoln) of mixing are always positive. (B) both the enthalpy (AHsoln) and the entropy (ASsoln) of mixing are always negative. (C) the enthalpy (AHsoln) is always negative, while the entropy (Scoln) is always positive. (D) the enthalpy (AHsoln) may be positive or negative, but the entropy (ASsoln) is always positive. (E) the enthalpy (AHsoln) is always negative, but the entropy (ASsoln) may be positive or negative.