0.1 mole of liquid ethanol C;H;OH was burned in a bomb calorimeter with a heat capacity of27.34 kJ.K. The temperature of the calorimeter was increased from 21.4°C to 26.4°C.a) Calculate the standard enthalpy change of combustion in kJ/mol.b) Calculate the standard enthalpy of formation for liquid C;H;OH in kJ/mol.c) For ethanol, AvapH° = 43.5 kJ/mol. Calculate q, w, AH and AU when 1.75 moleC;H;OH (I) is vaporized at 260 K and 765 Torr.AH° / kJ.molH20(g)H20(1)CO2(g)-241.82-285.83-393.51Suppose you have 1 mole of a monatomic ideal propane (C3H3) at 1bar and 300 K. Calculate q, w, AH and AU for each of the processes described in part a, b, and c.a) The system undergoes a reversible isothermal expansion until its volume is tripled.b) The system undergoes an irreversible expansion until its volume is tripled and against an external pressureof 0.1 bar.c) The system undergoes a reversible process in which 1 kJ of heat is absorbed by the gas and theenthalpy change is -1.50 kJ."he molar volume of vapor water at 327.6 atm and 776.4 K is 1.35x10* m mol.a) given that a = 5.464 dm, calculate the parameter b in the van der Waals equation of vapor water.b) calculate the compression factor of vapor water.c) accordingly with your answer to b), is it easier to compress vapor water or a perfect gas?d) accordingly with your answer to b), what type of interactions (i.e., attractive or repulsive) dominate invapor water under these conditions?e) the van der Waals equation can be expanded in a power series to yield its virial form as follows:(b- *a1pVm = RT 1++ b2.+RT VmUsing this expression, calculate an approximate value of the compression factor by including only thefirst three term in the virial expansion of the van der Waals equation.

Answered: Image /qna-images/answer/f18e1f30-96c4-4fb4-8b0f-d8e5da2da6be.jpg

0.1 mole of liquid ethanol C;H;OH was burned in a bomb calorimeter with a heat capacity of 27.34 kJ.K!. The temperature of the calorimeter was increased from 21.4°C to 26.4°C. a) Calculate the standard enthalpy change of combustion in kJ/mol. b) Calculate the standard enthalpy of formation for liquid C;HsOH in kJ/mol. c) For ethanol, AvapH° = 43.5 kJ/mol. Calculate q, w, AH and AU when 1.75 mole C;HŞOH (I) is vaporized at 260 K and 765 Torr. AH° / kJ.mol H2O(g) H20(I) CO2(g) -241.82 -285.83 -393.51 Suppose vou have 1 mole of a monatomic ideal propane (C:Hs) at 1

0.1 mole of liquid ethanol C;H;OH was burned in a bomb calorimeter with a heat capacity of 27.34 kJ.K!. The temperature of the calorimeter was increased from 21.4°C to 26.4°C. a) Calculate the standard enthalpy change of combustion in kJ/mol. b) Calculate the standard enthalpy of formation for liquid C;HsOH in kJ/mol. c) For ethanol, AvapH° = 43.5 kJ/mol. Calculate q, w, AH and AU when 1.75 mole C;HŞOH (I) is vaporized at 260 K and 765 Torr. AH° / kJ.mol H2O(g) H20(I) CO2(g) -241.82 -285.83 -393.51 Suppose vou have 1 mole of a monatomic ideal propane (C:Hs) at 1

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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