assuming that the densities of water in all phases are 1g/mL and that the Cp (J/K-mole) for ice and steam is 37.7 and 75.3 for liquid water, the total enthalpy change in heating 180 grams of ice at -5°C to steam at 105 °C is ____KiloJoules.

Suppose you have a perfectly insulated container holding 2.00 kg of liquid water at a temperature of 20.0°C. You also have a large supply of ice cubes which are stored at a temperature of-20.0°C. (a) What is the maximum mass of ice you can add to the water so that all of the ice melts? Assume no heat is lost to the environment. (b) Suppose you add twice the mass of ice that you found in part a. How much solid ice will remain once thermal equilibrium is reached?

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.05  kg of water decreased from 117  °C to 56.5  °C.  Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C

kJ. The specific heats of ice, water, and The enthalpy change for converting 1.00 mol of ice at -50.0 °C to water at 60.0°C is steam are 2.09 J/g-K, 4.18 J/g-K, and 1.84 J/g - K, respectively. For H₂O, A Hfus = 6.01kJ/mol, and AHvap = 40.67 kJ/mol. 6401 12.28 12.41 6.37 8.64

Calculate the enthalpy change upon converting 45g of steam at 150 C to ice at -30 C under a constant pressure of 1 atm. The specific heats of ice, liquid water, and steam are 2.03, 4.18, and 1.84 J/g-K, respectively.

If 100.0 g of water at 15.0 °C is poured over 15.50 g of ice at 0.0 °C, will all of the ice melt? Justify your answer and include any pertinent calculations. The molar mass of H2O is 18.02 g/mol. Table 1: Thermal data for waterConstant ValueHeat Capacity of Steam (Cp, H2O(g)) 2.01 g/J°CHeat Capacity of Liquid Water (Cp, H2O(l)) 4.18 g/J°CHeat Capacity for Ice (Cp, H2O(s)) 2.09 g/J°CHeat of Vaporization of Water (ΔHvap) 40.7 kJ/molHeat of Fusion for Water (ΔHfus) 6.02 kJ/mol

Pentane C5H12 boils at 360C at 1 atmosphere pressure. What is the molar heat of vaporization in kJ/mol if the vapor pressure of pentane at 250C is 505 torr?

Based on the thermodynamic properties provided for water, determine the energy change when the temperature of 1.45  kg of water decreased from 109  °C to 40.5  °C.   Property Value Units Melting point 0 °C Boiling point 100.0 °C ΔHfus 6.01 kJ/mol ΔHvap 40.67 kJ/mol cp (s) 37.1 J/mol · °C cp (l) 75.3 J/mol · °C cp (g) 33.6 J/mol · °C      kJ

Calculate the quantity of heat required to convert 70.5 g of H2O(s) at -25°C to H2O(g) at 125°C. fusH of ice at 0°C is 333 J g-1 vapH of liquid water at 100°C is 2260 J g-1 Specific heat capacity of H2O(s) = 2.06 J g-1 K -1 Specific heat capacity of H2O(l) = 4.184 J g -1 K -1 Specific heat capacity of H2O(g) = 1.92 J g-1 K -1 answer in KJ