Calculate the molar entropy (on a degree of freedom basis) of N2O at 298K, p = 1atm (QRot = 0.603 and QVib = 3200, 850(2), 1840, s = 1, and g0 = 1). Which degree of freedom contributes the most to the total entropy? How does the total entropy compare to the experimental value of 220.1 J/K/mol?

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11 Dec 2019

Calculate the molar entropy (on a degree of freedom basis) of N₂O at 298K, p = 1atm (Q_Rot = 0.603 and Q_Vib = 3200, 850(2), 1840, s = 1, and g₀ = 1). Which degree of freedom contributes the most to the total entropy? How does the total entropy compare to the experimental value of 220.1 J/K/mol?

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Q1. Boiling points Taking the last digit of your student ID number as a key, select the corresponding solvent from the table below. Assume you are using that solvent for the following questions. solve the first one Carbon disulphide

ID numbe	Solvent	boiling point (1 atm)	ÎvapHÂ° / Â°C /kJ mol-1
0,1	Carbon disulphide	46.3	26.7
2,3	Carbon tetrachloride	76.7	30.0
4,5	Cyclohexane	80.7	30.1
6,7	Diethylether	34.6	27.1
8,9	Acetone	56.0	31.3

(a) Compute the entropy of vaporisation of this solvent. (Briefly, compare the value you obtain with that from Troutonâs rule (ÎvapSÂ° â10.5 R). answer this qustion)

Entropy of vaporization= 0.08362 kJ mol^-1/K

Entropy of vaporization= 83.62 J mol^-1/K

(b) Use the tabulated experimental value of ÎvapHÂ° to estimate the partial pressure (i.e. vapour pressure, in atm) of that solvent at room temperature (25 Â°C). What implications does this have for safe storage and handling of the solvent?answer this qustion)

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Calculate the molar entropy (on a degree of freedom basis) of N₂O at 298K, p = 1atm (Q_Rot = 0.603 and Q_Vib = 3200, 850(2), 1840, s = 1, and g₀ = 1). Which degree of freedom contributes the most to the total entropy? How does the total entropy compare to the experimental value of 220.1 J/K/mol?

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