Please correct answer and don't use hand raiting (a) If a sample of 2.0 mol of helium gas (assume ideal gas) is isothermally and reversiblyexpanded at 300 K from a pressure of 2.5 bar to a pressure of 1,0 bar, find w and q. (b) Ifthe sample of helium from part (a) is isothermally and irreversibly expanded from thesame initial state to the same final state with Pext = 1.0 bar, find w and q. (10%)of SO₂ is described by the following equation over theC

For equations to write and integration symbol, I am using hand written solution. I will try to write…

Answered: (a) If a sample of 2.0 mol of helium…

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter13: Spontaneous Processes And Thermodynamic Equilibrium

Section: Chapter Questions

Problem 16P

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Calculate the standard Gibbs free-energy change when SO3 forms from SO2 and O2 at 298 K. Why is sulfur trioxide an important substance to study? (Hint: What happens when it combines with water?)
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.
A 220-ft3 sample of gas at standard temperature and pressure is compressed into a cylinder, where it exerts pressure of 2000 psi. Calculate the work (in J) performed when this gas expands isothermally against an opposing pressure of 1.0 atm. (The amount of work that can be done is equivalent to the destructive force of about 1/4 lb of dynamite, giving you an idea of how potentially destructive compressed gas cylinders can be if improperly handled!)
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the formation of hydrogen sulfide from the elements? H2(g)+18S8(s)H2S(g)
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?
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.
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).
What is the sign of the standard Gibbs free-energy change at low temperatures and at high temperatures for the explosive decomposition of TNT? Use your knowledge of TNT and the chemical equation, particularly the phases, to answer this question. (Thermodynamic data for TNT are not in Appendix G.) 2C7H5N3O6(s) 3N2(g) + 5H2O() + 7C(s) + 7CO(g)
Use the two appropriate values of R to determine a conversion between L. atm and J.
Billions of pounds of acetic acid are made each year, much of it by the reaction of methanol with carbon monoxide. (AssumeT= 298 K.) CH3OH() + CO(g) CH3COOH() (a) By calculating the standard Gibbs free energy change, rG, for this reaction, show that it is product-favored. (b) Determine the standard Gibbs free energy change, rG,for the reaction of acetic acid with oxygen to form gaseous carbon dioxide and liquid water. (c) Based on this result, is acetic acid thermodynamicallystable compared with CO2(g) and H2O()? (d) Is acetic acid kinetically stable compared with CO2(g)and H2O()?
What is the finaltemperature of0.122 mole ofmonatomic ideal gas that performs 75J of work adiabatically if the initial temperature is 235C?

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