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11) The enthalpy of vaporization of hydrogen sulfide, H2S, at its boiling point under standard pressure,...
the normal boiling point of ethanol is 78.3 deg C and its molar enthalpy of vaporization is 38.56 Kj/mol. what is the change in entropy in the system in J/k when 97.2 grams of ethanol at 1 atm condenses to a liquid at the normal boiling point?
Trouton's rule states that the molar enthalpy of vaporization of a liquid that does not have strong molecular interactions such as hydrogen bonding or ion-ion attractions is given by Boiling Chemical Compound formula AH yap (kJ-moll) point Hus (kJ.mol-) (K) chloromethane CH CI 21.40 249.06 6.43 water HO 40.65 373.15 6.01 hydrogen H,S 18.67 213.60 18.67 sulfide A Hvap = (85J.K-. mol-?)T where T, is the normal boiling point of the liquid in kelvins. Apply Trouton's rule to estimate the...
The normal boiling point of acetone [(CH3)2CO; MW 58.08 g/mol] is 56.1°C, and its molar enthalpy of vaporization is 29.1 kJ/mol. What is the molar entropy of vaporization of 72.3 g of acetone? molar ΔSvap = _____ J/(mol•K) What is the total entropy of vaporization of 72.3g of acetone? total ΔSvap = J/K
The enthalpy of vaporization of trichloromethane (chloroform, CHC13) is 29.4 kJ mol-'at its normal boiling point of 334.88 K, calculate (i) the entropy of vaporization of trichoromethane at this temperature and (ii) the entropy change of the surrounding.
The normal molar vaporization enthalpy (∆H_Vap ^ °) of methanol is worth 37.4 kJmol ^ (- 1), and its normal molar vaporization entropy (∆S_Vap ^ °) 110.9 JK ^ (- 1) mol ^ (- 1). Calculate: The vapor pressure of methanol, at 298 K (R = 8.3144 J K -1 mol -1). The approximate normal boiling point. The boiling point for an external pressure of 0.1 atm. Applying the Clausius-Clapeyron equation, estimate the cooking temperature in a pressure cooker whose...
196 The normal boiling point of Br2(l) is 58.8 ∘C, and its molar enthalpy of vaporization is ΔHvap = 29.6 kJ/mol. a) When Br2(l) boils at its normal boiling point, does its entropy increase or decrease? b) Calculate the value of ΔS when 1.50 mol of Br2(l) is vaporized at 58.8 ∘C. ΔS= (answer in J/K)
The molar enthalpy of vaporization of hexane (C6H14) is 28.9 kJ/mol, and its normal boiling point is 68.73°C. What is the vapor pressure of hexane at 25°C? (R-8.314 J/K • mol) O 4.44 torr O 117 torr O 171 torr O 759 torr 0 3370 torr
Can you show the work for these problems? Ethanol has an enthalpy of vaporization of 42.3 kJ/mol. The compound has a vapor pressure of 1.00 atm at 78.3 degree C. At what temperature is the vapor pressure equal to 0.800 atm? (R = 8.314 J/K middot mol) -83.8 degree C -24.4 degree C 62.6 degree C 73.0 degree C 78.0 degree C A liquid has an enthalpy of vaporization of 30.4 kJ/mol. At 269 K is has a vapor pressure...
The vaporization of compound A is described by the following chemical equation. A(1) A(8) A rap(72.39 °C) = 38.21 kJ/mol Calculate the entropy of vaporization, Aswap, for A(l) at 25.0 °C given that the boiling point of A is 72.39 °C, and the molar heat capacity of A(l) is 119.09 J/mol K). Assume that the molar heat capacity of A(R) is 56.5% of that of A(1). ASP J. mol-K Calculate the standard enthalpy of vaporization. A Hap, for A(1) at...
The normal boiling point of ammonia is -33.3°C, and its enthalpy of vaporization is 23.35 kJ/mol. Calculate the temperature in °C required to double the vapor pressure of ammonia.