5.30 The average enthalpy change of vaporization of benzenebetween room temperature and the normal boilingtemperature is 34.085 kJ mol-1. The vapor pressure at26.1°C is 100.0 torr.a. Find the normal boiling temperature. Compare with thecorrect value, 80.1°C. State any assumptions.b. Find the entropy change of vaporization at the normalboiling temperature. Compare with the prediction ofTrouton's rule. State any assumptions.

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Answered: 5.30 The average enthalpy change of…

Chemistry

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Chapter17: Spontaneity, Entropy, And Free Energy

Section: Chapter Questions

Problem 84AE: Calculate the entropy change for the vaporization of liquid methane and liquid hexane using the...

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In the thermodynamic definition of a spontaneous process, why is it important that the phrase “continuous intervention” be used rather than just “intervention?”
Calculate the entropy change for the vaporization of liquid methane and liquid hexane using the following data. Boilling point (1atm) Hvap Methane 112K 8.20 KJ/mol Hexane 342K 28.9 KJ/mol Compare the molar volume of gaseous methane at 112 K with that of gaseous hexane at 342 K. How do the differences in molar volume affect the values of Svap for these liquids?
The evaporation of one mole of water at 298 K has a standard free allergy change of 8.58 kJ. H2O(l)H2O(g)G298=8.58kJ (a) Is the evaporation of water under standard thermodynamic conditions spontaneous?. (b) Determine the equilibrium constant, KP, for this physical process. (c) By calculating G, determine if the evaporation of water at 298 K is spontaneous when the partial pressure of water, PH2O, is 0.011 atm.. (d) If the evaporation of water were always nonspontaneous at room temperature, wet laundry would never dry when placed outside. In order for laundry to dry, what must be the value of PH2O in the air?
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The free energy change, G, for a process at constant temperature and pressure is related to Suniv and reflects the spontaneity of the process. How is G related to Suniv? When is a process spontaneous? Nonspontaneous? At equilibrium? G is a composite term composed of H, T, and S. What is the G equation? Give the four possible sign combinations for H and S. What temperatures are required for each sign combination to yield a spontaneous process? If G is positive, what does it say about the reverse process? How does the G = H TS equation reduce when at the melting-point temperature of a solid-to-liquid phase change or at the boiling-point temperature of a liquid-to-gas phase change? What is the sign of G for the solid-to-liquid phase change at temperatures above the freezing point? What is the sign of G for the liquid-to-gas phase change at temperatures below the boiling point?
A reaction has H298=100 kj/mol and S298=250 J/mol K. Is the reaction spontaneous at room temperature? If not, under what temperature conditions will it become spontaneous?
The enthalpy of vaporization of ethanol is 38.7 kJ/mol at its boiling point (78C). Determine Ssys, Ssurr, and Suniv when 1.00 mole of ethanol is vaporized at 78C and 1.00 atm.
Given that H f for HF(aq) is -320.1 kJ/mol and S for HF(aq) is 88.7 J/mol K, find Ka for HF at 25C.
Consider two processes: sublimation of I2(s) and melting of I2(s) (Note: the latter process can occur at the same temperature but somewhat higher pressure). I2(s)I2(g)I2(s)I2(l) Is S positive or negative in these processes? In which of the processes will the magnitude of the entropy change be greater?
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