kJ. The specific heats of ice, water, and steam are 2.09 J/g – K, 4.18 J/g - K, The enthalpy change for converting 1.00 mol of ice at -50.0 °C to water at 80.0°C is and 1.84 J/g – K, respectively. For H20, A Hfus = 6.01kJ/mol, and AHvap = 40.67 kJ/mol. 13.91 12.28 10.15 6.45 7906 O O O O O

Based on the thermodynamic properties provided for water, determine the amount of energy released for 130.0  g of water to go from 89.0 °C to -12.0 °C.  Property Value Units Melting point 0.0 °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

1. Calculate the amount of heat (in kJ) released when converting 150.2 g of water to ice at -23 degrees Celsius.    2. A closed vessel of volume 10.0 L initially contains 1.303 g of water and no water vapor. Please calculate the mass of liquid water remaining once the system reaches equilibrium at 30 degrees Celsius. The vapor pressure of water at that temperature is equal to 0.0418 atm.   3. A person drinks four glasses of cold water (5 degrees C) every day. The volume of each glass is 195. mL. How much heat (in kJ) does the body have to supply to raise the temperature of the water to 37 degrees C (body temperature)?   4.From these data: N2H4(l) + O2(g) à 2N2(g) + 2H2O(l) H= -622.2 kJ/mol H2(g) + ½O2 à H2O(l) H= -285.8 kJ/mol H2(g) + O­2(g) à H2O2(l) H= -115 kJ/mol Find H for the reaction:                 N2H4(l) + 2H2O2(l) à 2N2(g) + 4H2O(l)   5. Consider the following chemical equation. CH4(g) + 2O2(g) à CO2(g) + 2H2O(l)                 Using the values in the table, calculate…

What amount of heat (in kJ) is required to convert 15.5 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)