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- Given that ΔHo(fusion) of water is 6025 J/mol, Cp,m(ice) = 37.7 J K–1 mol–1, and Cp,m(water,liquid) = 75.3 J K–1 mol–1, calculate ΔG (in J) for the freezing of 68 moles of water at 1 atm pressure and the constant temperature T = 7.6 °C.alculate ΔS per mole for the melting of H2O at 0.°C, ΔHfus = 6.0 kJ/mol. J/mol·K1 mol of toluene, at 1 atm is heated up from 25ºC to 35ºC. How much heat do we need for that? Which is the enthalpy change of the process? (use: (�H/�V)p. Assume the pressure does not change. Data: cp = 0.405 cal/(g º), ρ = 0.8669 g/cm3 eta =1.0 x 10-3 K-1.
- The combustion of ethanol used as a fuel has the ff reaction: C2H5OH(g) + O2 (g) -> CO2(g) +H2O with heating values of HHV=-2960 kJ/kg and LHV =-20760 kJ/kg. What is the vaporization of H2O in kj/kg a. 2260 b. 6780 c. 2970 d.8910Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 791.0 g sample of acetone sitting in the lab has a temperature of 21.7°C. How much heat would be involved in lowering the temperature of the acetone to -200.0°C? (answer in Joules)The vaporization of 1 mole of liquid water (the system) at 100.9°C, 1.00 atm, is endothermic. H2O(l)+40.7kJH2O(g)Assume that at exactly 100.0°C and 1.00 atm total pressure, 1.00 mole of liquid water and 1.00 mole of water vapor occupy 18.80 mL and 30.62 L, respectively. Calculate the water's change in internal energy.
- The heat of vaporization for 1.0 mole of water at 100.°C and 1.0 atm is 40.55 kJ/mol. Calculate DS for the process H2O(l) -> H2O(g) at 100.°C.Unit 3: The normal boiling point of methanol is 64.7 °C and the molar enthalpy of vaporization is 71.8 kJ/mol. Assuming that the vaporization is an equilibrium process, what is the value of ΔS (in J mol-1 K-1) when 1.00 mol of CH3OH (l) vaporizes at 64.7 °C ?Calculate the entropy and enthalpy of vaporization for 1 mole of water at room temperature (25oC) and 1 atm from these thermodynamic data:Cm,p(H2O, liquid) = 75.29 J/K·mol, Cm,p(H2O, gas) = 33.58 J/K·mol and ∆vapH(H2O) = 40700 J/ mol (at 100oC)
- Formula: C3H6OMelting Point: -94.0°CBoiling Point: 56.0°CDensity of liquid: 0.791 g/mLHeat of Fusion: 98.14 J/gHeat of vaporization: 538.9 J/gSpecific heat capacity (solid): 1.653 J/g°C Specific heat capacity (liquid): 2.161 J/g°C Specific heat capacity (gas): 1.291 J/g°C A 523.70 g sample of acetone gas has a temperature of 56.0°C. How much heat is involved in converting it to a solid that has a temperature of -94.0°C? (Answer in Joules)The standard heat of formation for Ag2CrO4(s) is -712 kJ/mol at 298 K. Write the formation equation for Ag2CrO4(s) that goes with this value of ΔH°.Be sure to specify states. Write fractions with a slash, such as 1/2 for one half.Calculate ΔSvap for hydrogen sulfide from the following data: normal boiling point of H2S: -60.7oC ΔHvap of H2S: 18.7 kJ/mol Place ΔSvap in units of J/(mol K) and your answer should have 3 significant figures.