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

Physical Chemistry

2nd Edition

ISBN:9781133958437

Author:Ball, David W. (david Warren), BAER, Tomas

Publisher:Ball, David W. (david Warren), BAER, Tomas

Chapter4: Gibbs Energy And Chemical Potential

Section: Chapter Questions

Problem 4.1E: List the sets of conditions that allow dS, dU, and dH of a process in a system act as a spontaneity...

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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.
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…
Use the calibration curve data provided to determine the entropy (ΔS, in J/K) associated with dissolving KNO3. please put the answer in this format: ____x10___power ___units *use correct sig figs
Benzene (C6H6) has a melting point of 5.50C and an enthalpy of fusion of 10.04kJmol-1 at 25.00C. The molar heat capacities at constant pressure for solid and liquid benzene are 100.4JK-1mol-1 and 133.0JK-1mol-1, respectively. Calculate the change of entropy of system and change of entropy of the surrounding at 100C for the reaction of C6H6(l)---->C6H6(s)
1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure. a) Calculate entropy change of the system, surrounding and universe. (temperature of the environment is -10 °C) b) Make some comments on entropy changes from the obtained data Please use the following data for water : Melting entalpy of ice (ΔHmelting) at 0°C and 1 bar is 6020 J mol-1. Cp (H2O (s)) = 37,7 J mol-1 K-1 Cp (H2O (l)) = 75,3 J mol-1 K-1
(a)At 0 oC, liquid water and ice are in equilibrium at standard pressure, so they have the SAME molar Gibbs energy. When raise from 1.0 bar to 100 bar, how much Gibbs free energy change in the liquid phase ? (molar mass of water 18 g mol-1; mass density of ice = 0.9150 g cm-3; mass density of liquid water, 0.9999 g cm-3) Set the initial Gibbs energy = 0 if you like. (b) how much Gibbs free energy change in the solid phase? c) under this process according to your calculation , solid changes to liquid. Liquid changes to solid
Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50 g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40 g of ethylbenzene (PhEt) and 50 g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead you mix 40 g of benzyl alcohol (PhMeOH) into 50 g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as:ΔΔG = ΔmixG[ PhMeOH ∶ PhH ] − ΔmixG[ PhEt ∶ PhH ]What do you expect the sign of ΔΔG to be? ( ΔΔG < 0, ΔΔG ≈ 0, or ΔΔG > 0 )Briefly justify your answer.
For the complete neutralization reaction between a 1 M strong acid and a 1 M strong base of equal initial volumes that is marked by a temperature rise, the entropy of neutralization is positive (ΔSrxn > 0) whereas the Gibbs free energy is negative (ΔGrxn < 0). Is this true or false? Please explain.
Assume that solutions of ethylbenzene : benzene behave ideally. a) Calculate the entropy of mixing if 40 g of ethylbenzene is mixed into 50g of benzene.b) At room temperature (298 K), what is ΔmixG for mixing 40g of ethylbenzene (PhEt) and 50g of benzene (PhH)?c) Would you notice a temperature change associated with the process in parts a) & b)?d) Instead, you mix 40g of benzyl alcohol (PhMeOH) into 50g of benzene (PhH). Let’s denote the difference between this process and the process in part b) as: ΔΔG = ΔmixG [PhMeOH ∶ PhH] − ΔmixG [PhEt ∶ PhH] What do you expect the sign of ΔΔG to be? (ΔΔG<0, ΔΔG≈0, or ΔΔG>0)Briefly justify your answer.
A closed, but not isolated system is in thermal contact with its surroundings. The system's volume is fixed at 7.3 L. Both the system and surrounds have a temperature of 25 °C. A chemical reaction occurs inside the system for which ΔrU = 11.38 KJ. (A) What is the change in entropy for the surroundings for the process, ΔSsurr? (B) What are the ranges of possible values for the change in entropy of the system, ΔSsys , for this process?
The boiling point of water at p = 1.0 atm is 100°C and its enthalpy of vaporization is delta Hvap = 40.7 kJ mol-1. Calculateq, w and delta Uand delta S for the process in which 2.0mol of water is vaporized at 100°C and p=1.0atm
P3B.7 A block of copper of mass 500 g and initially at 293K is in thermalcontact with an electric heater of resistance 1.00 kΩ and negligible mass. Acurrent of 1.00A is passed for 15.0 s. Calculate the change in entropy of thecopper, taking Cp,m = 24.4 JK−1mol−1. The experiment is then repeated with thecopper immersed in a stream of water that maintains the temperature of thecopper block at 293K. Calculate the change in entropy of the copper and thewater in this case.P3B.8 A block of copper (Cp,m = 24.44 JK−1mol−1) of mass 2.00 kg and at0 °C is introduced into an insulated container in which there is 1.00molH2O(g) at 100 °C and 1.00 atm. Assuming that all the vapour is condensed toliquid water, determine: (a) the final temperature of the system; (b) the heattransferred to the copper block; and (c) the entropy change of the water, thecopper block, and the total system. The data needed are given in ExerciseE3B.7a.