Determine the enthalpy of vaporization, in kJ/mol, of H₂O if 20.4 kJ of heat is needed to vaporize 0.500 moles of H₂O.
Determine the enthalpy of vaporization, in kJ/mol, of H₂O if 20.4 kJ of heat is needed...
222.The enthalpy of vaporization for chlorine is 20.41kJ/mol. How much heat is required to vaporize 293.39g of chlorine liquid at its boiling point? Report your answer in units of kJ.
1. a. The enthalpy of vaporization of liquid mercury is 59.11 kJ/mol. What quantity of energy as heat is required to vaporize 0.240 mL of mercury at 357 °C, its normal boiling point? The density of mercury is 13.6 g/mL. Energy = ____ kJ b. Determine ethanol’s normal boiling point by slowly changing the temperature to the point where the vapor pressure equals 760 mmHg. What is this temperature? °C
2)) Find the heat of fusion (H°) for a substance whose heat of sublimation is 38 kJ/mol and heat of vaporization is 23 kJ/mol. 2)) Find the heat of fusion (H°) for a substance whose heat of sublimation is 38 kJ/mol and heat of vaporization is 23 kJ/mol.
The heat of vaporization of benzene c6h6 , is 30.8 kJ/mol at its boiling point of 80.1 degrees Celsius. How much energy in the form of heat is required to vaporize 128 g benzene at its boiling point?
The heat of vaporization of benzene, C6H6 is 30.7 kJ/mol at its boiling point of 80.1 C. How much energy in the form of heat is required to vaporize 132 g benzene at its boiling point? a) 0.302 kJ b) 51.9 kJ c) 24.2 kJ d) 40.1 kJ c) 4.05 x 10^3 kJ
3. The heat of vaporization of a compound is 512 kJ/mol. When 1.28 mol of this compound vaporize at standard pressure, the entropy increases from 1243 J/K to 1751 J/K. What is the melting point of this compound at standard pressure to three significant figures? A) 1290 K B) 1010 K C) 787 K D) 292 K E) 412 K
How much heat is needed to vaporize 225 g of rubbing alcohol C3H8O at its boiling point? The enthalpy change of vaporization of rubbing alcohol = 0.664 kj/mol.
Thermodynamics 1) The enthalpy of vaporization of water ∆H = -25 kJ mol-1 at T = 45 °C. When water V = 15 cm3 in an open vessel evaporates at this temperature, calculate the change in entropy of the surroundings. 2) For a given reaction, ∆H = 25 kJ and ∆S = 50 J/K. Above what temperature will this reaction occur spontaneously? 3) At T = 15°C a certain protein denatures reversibly with ∆H = 30 kJ/mol. The system is...
The standard enthalpy of vaporization (H°vap) of methylacrylate (CH2CHCO2CH3) is 36.0 kJ/mol. The normal boiling point of methylacrylate is 80.5°C. Calculate the vapour pressure of methylacrylate at 43.0°C.
What is a liquid's heat of vaporization? It is the amount of heat needed to vaporize one liter of the liquid at its boiling point. It is the amount of heat needed to melt one gram of the liquid at its freezing point. It is the amount of heat needed to vaporize one gram of the liquid at its boiling point. It is the amount of heat needed to vaporize one kg of the liquid at its boiling point.