1-(25 P.) A sample consisting of 4.00 mol He is expanded isothermally at 30 °C from 12.3 dm³ to 42.2 dm³ a) reversibly, b) against a constant external pressure equal to the final pressure of the gas, and c) freely (against zero external pressure). For the three processes calculate q, w, AU, and AH. (R-8.3145 J K¹ mol¹) IT Sales (5)

1-(25 P.) A sample consisting of 4.00 mol He is expanded isothermally at 30 °C from 12.3 dm³ to 42.2 dm³ a) reversibly, b) against a constant external pressure equal to the final pressure of the gas, and c) freely (against zero external pressure). For the three processes calculate q, w, AU, and AH. (R-8.3145 J K¹ mol¹) IT Sales (5)

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter17: Chemcial Thermodynamics

Section: Chapter Questions

Problem 17.107QE: Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is...

See similar textbooks

Similar questions

For a liquid, which would you expect to be larger, Sfusion or Sevaporation? Why?
For the reaction BaCO3(s) BaO(s) + CO2(g), rG = +219.7 kJ/mol-rxn. Using this value and other data available in Appendix L, calculate the value of fG for BaCO3(s).
Which of the following quantities can be taken to be independent of temperature? independent of pressure? (a) H for a reaction (b) S for a reaction (c) G for a reaction (d) S for a substance
Would the amount of heat absorbed by the dissolution in Example 5.6 appear greater, lesser, or remain the same if the heat capacity of the calorimeter were taken into account? Explain your answer.
Describe why it is easier to use Gto determine the spontaneity of a process rather than S u
For the process H2O(l)H2O(g) at 298 K and 1.0 atm, H is more positive than E by 2.5 kJ/mol. What does the 2.5 kJ/mol quantity represent?
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.
From data in Appendix J, estimate (a) the boiling point of titanium(IV) chloride. (b) the boiling point of carbon disulfide, CS2, which is a liquid at 25 C and 1 bar.
When 1.000 g of ethylene glycol, C2H6O2, is burned at 25C and 1.00 atmosphere pressure, H2O(l) and CO2(g) are formed with the evolution of 19.18 kJ of heat. a Calculate the molar enthalpy of formation of ethylene glycol. (It will be necessary to use data from Appendix C.) b Gf of ethylene glycol is 322.5 kJ/mol. What is G for the combustion of 1 mol ethylene glycol? c What is S for the combustion of 1 mol ethylene glycol?
One mole of H2O(g) at 1.00 atm and 100.C occupies a volume of 30.6 L. When 1 mole of H2O(g) is condensed to 1 mole of H2O(l) at 1.00 atm and 100.C, 40.66 kJ of heat is released. If the density of H2O(l) at this temperature and pressure is 0.996 g/cm3, calculate E for the condensation of 1 mole of water at 1.00 atm and 100.C.
The enthalpy of vaporization for water is 40.65 kJ mol-1. As a design engineer for a project in a desert climate, you are exploring the option of using evaporative cooling. (a) If the air has an average volumetric heat capacity of 0.00130 J cm-3 K-1, what is the minimum mass of water that would need to evaporate in order to cool a 5 m? 5 m room with a 3 m ceiling by 5°F using this method? (b) Is this a spontaneous or nonspontaneous process?
If the heat capacity varies withtemperature, abetter form ofequation 2.9 isto solve q=TiTfnCT-t A 50.0-g sample of white phosphorus is heated from 298 K to 350K. If its molar heat capacity is CT- = 56.990.1202T J/mol.K, how much heat is needed?