For each system listed in the first column of the table below, decide (i 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 enoug 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 1.0 g of ammonium bromide O AS = 0 The ammonium bromide is dissolved (NH Br) and 2.0 L of pure water in the water. O As>0 at 41 °C. not enough information O As< 0 A mixture of helium (He) gas and An additional 2.0 L of pure CO, O As = 0 carbon dioxide (CO,) gas at 2 atm gas is added to the mixture, with the O As> 0 and 2°C. pressure kept constant at 2 atm. not enough information O AS <0 The seawater is passed through a reverse-osmosis filter, which O AS = 0 separates it into 750. mL of pure water and 250. mL of brine (very A liter of seawater at 15° C. O As > 0 not enough information salty water).

For each system listed in the first column of the table below, decide (i 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 enoug 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 1.0 g of ammonium bromide O AS = 0 The ammonium bromide is dissolved (NH Br) and 2.0 L of pure water in the water. O As>0 at 41 °C. not enough information O As< 0 A mixture of helium (He) gas and An additional 2.0 L of pure CO, O As = 0 carbon dioxide (CO,) gas at 2 atm gas is added to the mixture, with the O As> 0 and 2°C. pressure kept constant at 2 atm. not enough information O AS <0 The seawater is passed through a reverse-osmosis filter, which O AS = 0 separates it into 750. mL of pure water and 250. mL of brine (very A liter of seawater at 15° C. O As > 0 not enough information salty water).

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 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" butto the last column. System Change AS AS 0 not enough information AS 0 not enough information AS 0 2.0 L. not enough information
Consider the reaction 4NH3(g) +50₂(g) 4NO(g) + 6H₂O(g) for which AH = -905.2 k) and AS 180.5 J/K at 298.15 K. (1) Calculate the entropy change of the UNIVERSE when 1.639 moles of NH3(g) react under standard conditions at 298.15 K. ASuniverse yk (2) Is this reaction reactant or product favored under standard conditions? (3) If the reaction is product favored, is it enthalpy favored, entropy favored, or favored by both enthalpy and entropy? If the reaction is reactant favored, choose 'reactant favored'.
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 System Change AS O AS 0 3.0 L. not enough information O As 0 not enough information O AS 0 constant at 55.0 °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 Change AS AS 0 sucrose solution. not enough information O AS 0 both at 5 atm and 43°C. not enough information O 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 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 AS 0 water and 250. mL of brine (very salty water). not enough information O O O O
Please explain as much as possible. Why did you use the equation? Or what conditions did you see from the question? etc
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
c) Provide an example of a chemical or biochemical process that can't be described as enthalpy-driven or entropy-driven and briefly justify your answer. If you can't find a good example, make up a plausible example and briefly explain.
need help with this chemistry review
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 ||
Calculating Thermodynamic Values from an Equilibrium ConstantBackgroundAs discussed in lecture, the free energy for a reaction can be related to the equilibriumconstant through the formula below.K = e (-ΔG° / RT)Therefore if Kc for a reaction is known, Go can be determined, or vice versa. Furthermore, ifyou have the value for Go at two different temperatures, you can calculate H and S throughthe familiar equation for Gibbs energy below, since you have two unknowns but also twoequations.G = H – T SIn this lab you will be studying the solubility of borax (Na2B4O5(OH)4*8H2O), a slightly solublesodium salt, at two different temperatures. When solid borax is added to water, theequilibrium below is established.Na2B4O5(OH)4*8H2O (s) 2 Na+ (aq) + B4O5(OH)42- (aq) + 8 H2O(l)If you measure the concentrations for those substances that show up in the reaction quotient,then the Kc for the reaction at that temperature can be calculated. In this lab, theconcentration of borate ion…
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…