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.

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.

Physical Chemistry

2nd Edition

ISBN:9781133958437

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

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

Chapter2: The First Law Of Thermodynamics

Section: Chapter Questions

Problem 2.32E: Many compressed gases come in large,heavy metal cylindersthat are so heavy that they need a special...

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1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure. Calculate entropy change of the system, surrounding and universe. (temperature of the environment is -10 °C) 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
The standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are respectively -238.7 kJ/mol, - 285.8 kJ/mol, and -393.5 kJ/mol. Calculate the change in surrounding entropy (in J/K) when burning 13.6 g of methanol under a constant pressure of 1.000 atm at 25.00 oC (N.B., combustion is the reaction of a substance with oxygen molecule to produce water and carbon dioxide).
The standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are, respectively, -238.7 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol. Calculate the change in the entropy of the surroundings (in J/K) upon the combustion of 13.3 g of methanol under a constant pressure of 1.000 atm and a temperature of 25.00 oC. N.B. combustion is the reaction of this substance with molecular oxygen to produce water and carbon dioxide.
Pure water under the atmospheric pressure of 100,000 Pa is converted to steam at a temperature of 100 0C. What statement can you make regarding the relation between Gibbs free energy (or chemical potential) of water and steam at 100 0C, under atmospheric pressure. If the heat needed to vaporise 1 kg of water to steam at 100 0C is 2265 kJ/kg. Work out the difference between entropy of steam and water at the boiling temperature. b) If a small amount of salt 0.0002 mol is added to every 18 g of water, calculate the chemical potential change of water in the salt solution. c) Assuming that the chemical potential of water in the solution does not change much with pressure, work out the pressure at which the water in the salt solution will boil, at 100 0 You may take steam as being an ideal gas.
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 standard enthalpies of formation, at 25.00 oC, of methanol (CH4O(l)), water (H2O(l)), and carbon dioxide (CO2(g)) are -238.7 kJ/mol, -285.8 kJ/mol, and -393.5 kJ/mol respectively. Calculate the change in surrounding entropy (in J/K) during combustion of 12.7 g of methanol under a constant pressure of 1,000 atm at 25.00 oC (N.B., combustion is the reaction of a substance with molecular oxygen to produce water and carbon dioxide).
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)
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.
In the process you design, benzene is used as a solvent.You needed the following information for equipment design. These featurescalculatea. Molar volume of liquid at 1 bar and 5 oCb. Molar volume of steam at 4 bar and 172 oCc.When benzene is heated and compressed from 1 bar and 5 oC to 4 bar and 172 oCwhat is the change in molar enthalpy, entropy and internal energy
A 1 mol quantity of hydrogen gas sample was heated at constant pressure from a temperature of 300 K to 500 K. With the entropy transformation process as a function of temperature variation, the heat capacity equation at constant pressure was estimated , Cp = 6.9469 - 0.199 x 10-3 T + 4.808 x 10-7 T2 (J K-1mol-1). Determine the entropy change of the process.
The molar heat capacity of N2(g) in the range 200K to 400K is given by Cpm (J/Kmol)= 28.58+3.77*10^-3 (T/K). Given that the standard molar entropy of N2(g) at 298K is 191.6 J/Kmol, determine q, w, change in enthalpy (H), change in internal energy (U), and change of entropy of the system (Ssys) when the temperature is raised from 25C to 100C under a) constant pressure and b) constant volume.
Consider the following reaction: H2(g) + ½ O2 (g) ------> H2O (g) The standard enthalpy of formation of gaseous H2O at 298 K is -241.82 kJ mol-1. Calculate the value at 153 0C. Given Cp,m for H2O(g): 33.58 kJ mol-1; H2 (g): 28.84 kJ mol-1; O2 (g): 29.37 kJ mol-1. Assume heat capacities are independent of T. NOTE:answer in kilojoules per mole (kJ/mol)