I got -46.7 KJ for part a but +100 KJ for part b (the van der waals version), I probably missed a negative sign somewhere, this question is for both a and b Now consider the same expansion treating ethanol as a van der Waals gas. (Look up thevan der Waals parameters in E&R appendix Table 7.4). Generate an indicator diagram(ideally, combine this indicator diagram with the one above, so that both curves will bein the same graph.) Next, you will need to derive an expression for the work associatedwith isothermal expansions (or compressions) on a van der Waals gas. This equationwill be analogous to w = nRT In for an ideal gas. (Yes, you will need to work out anViintegral; see the Bonus Lesson 2 part B document for guidance, if necessary.) Calculateq, w, and AU for the expansion.[HINT: for determining AU, you should start with the total differential expression and think about howyou can determine the values of the various partial derivatives. In some cases, you have already workedwith these values for other examples, so you just need to incorporate the relevant specific quantities forthis case.] 2. A 20.00 mol sample of gaseous ethanol is held at 5.50 x 10² K in a cylinder with a piston setsuch that the volume is 12.00 L. The ethanol expands isothermally and reversibly to a finalvolume of 45.00 L.Consider ethanol as an ideal gas. Plot the relevant indicator diagram (Make life easier,use a spreadsheet! Be sure to follow the guidance provided in Bonus Lesson 2, part A!).Then, determine the value of the quantities q, w, and AU (signs are important!) for thisexpansion.

A 20.00 mol sample of ethanol at 5.50 × 102 K is expanded isothermally and reversibly from 12.00 L…

A 20.00 mol sample of gaseous ethanol is held at 5.50 x 10² K in a cylinder with a piston set such that the volume is 12.00 L. The ethanol expands isothermally and reversibly to a final volume of 45.00 L. Consider ethanol as an ideal gas. Plot the relevant indicator diagram (Make life easier, use a spreadsheet! Be sure to follow the guidance provided in Bonus Lesson 2, part A!). Then, determine the value of the quantities q, w, and AU (signs are important!) for this expansion.

A 20.00 mol sample of gaseous ethanol is held at 5.50 x 10² K in a cylinder with a piston set such that the volume is 12.00 L. The ethanol expands isothermally and reversibly to a final volume of 45.00 L. Consider ethanol as an ideal gas. Plot the relevant indicator diagram (Make life easier, use a spreadsheet! Be sure to follow the guidance provided in Bonus Lesson 2, part A!). Then, determine the value of the quantities q, w, and AU (signs are important!) for this expansion.

Chemistry

9th Edition

ISBN:9781133611097

Author:Steven S. Zumdahl

Publisher:Steven S. Zumdahl

Chapter6: Thermochemistry

Section: Chapter Questions

Problem 124CP: Consider 2.00 moles of an ideal gas that are taken from state A (PA = 2.00 atm, vA = 10.0 L) to...

See similar textbooks

Similar questions

Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.
What are the two ways that a final chemical state of a system can be more probable than its initial state?
When one mol of KOH is neutralized by sulfuric acid, q=56 kJ. (This is called the heat of neutralization.) At 23.7C, 25.0 mL of 0.475 M H2SO4 is neutralized by 0.613 M KOH in a coffee-cup calorimeter. Assume that the specific heat of all solutions is 4.18J/gC, that the density of all solutions is 1.00 g/mL, and that volumes are additive. (a) How many mL of KOH is required to neutralize H2SO4? (b) What is the final temperature of the solution?
On complete combustion at constant pressure, a 1.00-L sample of a gaseous mixture at 0C and 1.00 atm (STP) evolves 75.65 kJ of heat. If the gas is a mixture of ethane (C2H6) and propane (C3H8), what is the mole fraction of ethane in the mixture?
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.
Use the data in Table 2.2 to determine Hp T for Ar at 0C and 1atm. Make any reasonable assumptions necessary.
In the 1880s, Frederick Trouton noted that the enthalpy of vaporization of 1 mol pure liquid is approximately 88 times the boiling point, Tb, of the liquid on the Kelvin scale. This relationship is called Troutons rule and is represented by the thermochemical equation liquid gas H = 88 Tb, joules Combined with an empirical formula from chemical analysis, Troutons rule can be used to find the molecular formula of a compound, as illustrated here. A compound that contains only carbon and hydrogen is 85.6% C and 14.4% H. Its enthalpy of vaporization is 389 J/g, and it boils at a temperature of 322 K. (a) What is the empirical formula of this compound? (b) Use Troutons rule to calculate the approximate enthalpy or vaporization or one mole of the compound. Combine the enthalpy of vaporization per mole with that same quantity per gram to obtain an approximate molar mass of the compound. (c) Use the results of parts (a) and (b) to find the molecular formula of this compound. Remember that the molecular mass must be exactly a whole-number multiple of the empirical formula mass, so considerable rounding may be needed.
Explain why the high-temperature reservoir of a heat engine must, indeed, be higher in temperature than the low-temperature reservoir. Can it ever be the other way around?
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).
A 21.3-mL sample of 0.977 M NaOH is mixed with 29.5 mL of 0.918 M HCl in a coffee-cup calorimeter (see Section 6.6 of your text for a description of a coffee-cup calorimeter). The enthalpy of the reaction, written with the lowest whole-number coefficients, is 55.8 kJ. Both solutions are at 19.6C prior to mixing and reacting. What is the final temperature of the reaction mixture? When solving this problem, assume that no heat is lost from the calorimeter to the surroundings, the density of all solutions is 1.00 g/mL, the specific heat of all solutions is the same as that of water, and volumes are additive.
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?
What is the change in internal energy when a gas contracts from 377mL to 119mLundera pressure of 1550 torr, whileat the same time being cooled by removing 124.0J ofheat energy?