Calculate the enthalpy change in kJ upon converting 0.50 mol of water at 45.0oC to a water vapor at 175.0oC under constant pressure of 1 atm. The specific heats of ice, liquid water, and gaseous water are 2.09 J/gK, 4.18 J/gK, and 1.84 J/gK. The heat of fusion of water is 6.01 kJ/mol and the heat of vaporization of water is 40.67 kJ/mol.

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

Calculate the amount of energy (in kJ) necessary to convert 497 g of liquid water from 0°C to water vapor at 182°C. The molar heat of vaporization (Hvap) of water is 40.79 kJ/mol. The specific heat for water is 4.184 J/g °C, and for steam is 1.99 J/g °C. (Assume that the specific heat values do not change over the range of temperatures in the problem.) kJ

What amount of thermal energy (in kJ) is required to convert 221 g of ice at -16 °C completely to water vapour at 214 °C? The melting point of water is 0 °C and its normal boiling point is 100 °C. The heat of fusion of water is 6.02 kJ mol-¹ The heat of vaporization of water at its normal boiling point is 40.7 kJ mol-¹ The specific heat capacity of ice is 2.09 J g-¹ °C-¹ The specific heat capacity of liquid water is 4.18 J g-¹ °C-¹ The specific heat capacity of water vapour is 2.01 Jg¹¹ °C-¹ Answer:

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

Two 20.0 g ice cubes at -14.0 °C are placed into 295 g of water at 25.0 °C. Assuming no energy is transferred to or from the surroundings, calculate the final temperature, Tf, of the water after all the ice melts. heat capacity of H₂O(s) heat capacity of H₂O(1) enthalpy of fusion of H₂O 37.7 J/(mol.K) 75.3 J/(mol.K) 6.01 kJ/mol Tf= °C

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

When 5.00 g of isopropyl alcohol ((CH3),CHOH; molar mass = point of 82.6°C, it absorbs 3.66 kJ of heat. What is the enthalpy of vaporization of isopropyl alcohol in kJ/mol? 60.09 g/mol) evaporates at its boiling

at 100.0C the molar heat of vaporization of water is 40.67KJ/mol. at 25.0C approximately room temperature, the molar heat of vaporization of water is 44.0KJ/mol. during a strenuous work out, an athlete generates 2010KJ of heat energy. what mass of water would have to evaporate from the athletes skin to dissipate 2010KJ of heat? in grams

Chloroform, CHCl3 is a volatile liquid and has a boiling point of 61.7 ° C and has a heat of vaporization of 31.4 kJ/mol. What is the vapor pressure of chloroform at 37.2 °C?