Calculate the change in entropy of fusion when supercooled water at -3°C freezes at constant P and T. The molar enthalpy of fusion of ice is 6000 Jmol' at 0°C. The heat capacity of ice is 38 JK'mol".
Q: The enthalpy of vaporization of benzene at 1 atm and its normal boiling point 353 K is 30.8 kJ/mol.…
A: The enthalpy of vaporization of benzene is 30.8 kJ/mol. The boiling point of benzene is 353 K.
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Q: he molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1 , and the…
A: ΔfusHm (H2O)=6.01 kJ mol-1ΔfusSm (H2O)=22.0J K-1 mol-1
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Q: 1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure.…
A: GIVEN: Melting entalpy of ice=6020 J mol-1. n=1 mol super cooled liquid Freezing point =0 deg C =273…
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Q: the enthalpy of vaporization,
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Q: Calculate the entropy changes in the system and in the surroundings.
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- 1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure. Calculate entropy change of the system, surrounding and universe. (temperature of the environment is -10 °C) Please use the following data for water : Melting entalpy of ice (ΔHmelting) at 0°C and 1 bar is 6020 J mol-1. Cp (H2O (s)) = 37,7 J mol-1 K-1 Cp (H2O (l)) = 75,3 J mol-1 K-1The molar enthalpy of fusion of ice at 273.15 K and one atm is ΔfusHm (H2O)=6.01 kJ mol-1, andthe molar entropy of fusion under the same conditions is ΔfusSm (H2O)=22.0 J K-1 mol-1. Show that(a) ΔfusGm (H2O)=0 at 273.15 K and one atm, (b) ΔfusG,m (H2O) < 0 when the temperature is greaterthan 273.15 K, and (c) ΔfusGm (H2O) > 0 when the temperature is less than 273.15 K.1 mol super cooled liquid water transformed to solid ice at -10 oC under 1 atm pressure. a) Calculate entropy change of the system, surrounding and universe. (temperature of the environment is -10 °C) b) Make some comments on entropy changes from the obtained data Please use the following data for water : Melting entalpy of ice (ΔHmelting) at 0°C and 1 bar is 6020 J mol-1. Cp (H2O (s)) = 37,7 J mol-1 K-1 Cp (H2O (l)) = 75,3 J mol-1 K-1
- Find the molar entropy of vaporization of hexane (C6H14) given that at Pº=1 bar and T=69.0 ºC 2.52 kJ of heat is required to vaporize 7.53 g of hexaneThe enthalpy of vaporization (deltaHvap) of water was experimentally determined to be 151.3 kJ for 3.72 mols of water at 100 degrees Celsius? Calculate the molar entropy of vaporaization (deltaSvap,m) of water.The enthalpy of vaporization of benzene at 1 atm and its normal boiling point 353 K is 30.8 kJ/mol. What is the difference in entropy between gaseous and liquid benzene under these conditions?
- At 0 °C 20 g of ice are added to 50 g of water at 30°C in a vessel that has a water equivalent of 20 g. Calculate the entropy changes in the system and in the surroundings. The heat of fusion of ice at 0 C is 6.02 kJ mol, and the specific heat capacities of water and ice may be taken as constant at 4.184 and 2.094 J Kg, respectively, and independent of temperatureA sample of carbon dioxide that initially occupies 15.0 dm3 at 250 K and 1.00 atm is compressed isothermally. Into what volume must the gas be compressed to reduce its entropy by 10.0 J K-1?Two moles of liquid water at 25 ° C is placed in a freezer having a temperature of – 10 ° C. Calculate the change in entropy.Cp,m for liquid water = 75.3 J K-1 mol-1Cp,m for ice = 37.7 J K-1 mol-1For water, ΔΗfusion = 6.01 kJmol-1
- Calculate the change in entropy (in J/⁰F) when 340g of ethanol (46 g/mol) is cooled from 50 to 40 ⁰C at constant pressure. Specific heat capacity of methanol at constant pressure is 112 J/mol-K.Benzene (C6H6) has a melting point of 5.50C and an enthalpy of fusion of 10.04kJmol-1 at 25.00C. The molar heat capacities at constant pressure for solid and liquid benzene are 100.4JK-1mol-1 and 133.0JK-1mol-1, respectively. Calculate the change of entropy of system and change of entropy of the surrounding at 100C for the reaction of C6H6(l)---->C6H6(s)Liquid nitrogen, which has a boiling point of −195.79°C, is used as a coolant and as a preservative for biological tissues. Liquid nitrogen also freezes to a white solid at −210.00°C, with an enthalpy of fusion of 0.71 kJ/mol.What is its entropy of fusion?