The Cp,m of liquid and solid water in the -10 °C to 0 °C range is 76.065 J mol-1 K-1 and 37.656 J mol-1 K-1, respectively. For water at -10°C and 1.0 atm, ΔSfreeze = -20.56 J mol-1 K-1. Solve for the free energy change (ΔG) when 59.8g of supercooled water freezes at 1.00 atm and a) 0 °C J b) -10 °C J
The Cp,m of liquid and solid water in the -10 °C to 0 °C range is...
I would really appreciate your help. God bless you Question 4 The molar enthalpy of fusion of ice at 0 °C and 1 atm pressure is 6024 J mol. The molar heat capacities at constant pressure of ice and water are 37.65 J Kmol and 75.30 J Kmol respectively, and may be taken as constant over the temperature range 0 to -20°C. Consider 2 mole of liquid water supercooled to -20 °C, which is allowed to freeze isothermally from liquid...
The molar enthalpy of fusion of solid bismuth is 11.0 kJ mol-1, and the molar entropy of fusion is 20.2 J K-1 mol-1. (a) Calculate the Gibbs free energy change for the melting of 1.00 mol of bismuth at 575 K. kJ (b) Calculate the Gibbs free energy change for the conversion of 5.12 mol of solid bismuth to liquid bismuth at 575 K. kJ (c) Will bismuth melt spontaneously at 575 K? (d) At what temperature are solid and...
The vaporization of 1 mole of liquid water (the system) at 100.9°C, 1.00 atm, is endothermic. HL,0(1) + 40,7kJ + HO( 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 Part 1 (2.5 points) Calculate the work done on or by the system when 2.05 mol of liquid H2O vaporizes. Part 2 (2.5 points) Calculate the water's change in internal...
The Standard enthalpy of vaporization of water at 100.0 oC is 40.66 KJ*mol-1. The Cp,m values for the liquid and the vapor water are, respectively, 75.3 and 33.58 J*K-1*mol-1. Assume that the heat capacities are independent of temperature, and that the vapor behaves as an ideal gas. a) Calculate sys in taking one mole of liquid water at 25.0 oC and 1.00 atm to gaseous water at 95.0 oC and 0.500 atm. b) Assume that the temperature and pressure of...
The change in enthalpy when 1 mol of ice is melted at 273K is 6008 J Heat Capacity of liquid water, Cp_{L} = 75.44 J/mol K Heat Capacity of solid water, Cp_{S} = 38J/mol K Enthalpy chage of melting at 273K, \Delta H_{273}=6008 J Calculate the standard enthalpy of fusion for ice. Calculate the heat released when 100 g of water supercooled at 250K solidify Initial T=25°C=298K Thanks
The vaporization of 1 mole of liquid water (the system) at 100.9°C, 1.00 atm, is endothermic. H2O(l)+40.7kj -------> H2O(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. Part 1 Calculate the work done on or by the system when 1.25 mol of liquid H2O vaporizes. Part 2 Calculate the water's change in internal energy
Please just answer Part 2 The vaporization of 1 mole of liquid water (the system) at 100.9°C, 100 atm, s endothermic. H0HOg) 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 5th attempt d See Periodic Table See Hint (0.5 point) Part 1 Calculate the work done on or by the system when 1.85 mol of liquid H20 vaporizes. 5736.23319:J (0.5...
The enthalpy of fusion of cadmium at its normal melting point of 321 °C is 6.11 kJ mol? What is the entropy of fusion of cadmium at this temperature? ASfus = J mol-K-1 The molar enthalpy of fusion of solid cadmium is 6.11 kJ mol-1, and the molar entropy of fusion is 10.3 JK+mol-1. (a) Calculate the Gibbs free energy change for the melting of 1.00 mol of cadmium at 622 K. (b) Calculate the Gibbs free energy change for...
Gaseous H2O is condensed at 100°C and the liquid water is cooled to 0°C followed by freezing to solid water. What is the molar entropy change of the water? Consider the average specific heat of liquid water is 4.2 J/K g. The heat of vaporization at the boiling point and the heat of fusion at the freezing point at 2258.1 and 333.5 J/g, respectively.
An ice tray contains 490 g of liquid water at 0°C. Calculate the change in entropy of the water as it freezes slowly and completely at 0°C. J/K