For a given species, see the thermodynamic values below. Boiling Point: Melting Point: Heat of Vaporization: 90.0 C 10.0° C 30.0 kJ/mol Heat of Fusion: 10.0 kJ/mol heat capacity (solid): heat capacity (liquid): heat capacity (gas): 100.0 J/mol K 120.0 J/mol K 80.0 J/mol K Calculate the energy released in kJ as a 2.0 mol sample of benzene at 100°C is cooled to 50°C Report in kJ, do not use scientific notation. Give answer to the tenths place

53. What mass of water initially at -12.5 °C can be converted to liquid water at 27.9 °C by 38.36 kJ of energy? AHfus = 334 J/g AHvap =2261 J/g Csolid=2.11 J/g.°C Cliquid 4.18 J/g °C Cgas = 2.01 J/g °C A. 80.4 g B. 91.5 g C. 76.3 g D. 268 g =

• At its boiling point (-61 C), what mass of H2S is vaporized with 100 kJ? The AHvap of H2S, is 18.8 kJ/mol?

How much heat energy is required to convert 65.6 g of solid iron at 27 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g- °C). q= kJ

instant pan pressure cooker has an enthalpy of vaporization of water 40.67 kJ/mole. calculate the boiling temperature C of water inside a pressure pan cooker that has been pressurized to 5.9 atm.

Calculate the heat change in joules for vaporization of 9.00 g of water at 100 ∘C.

How much heat energy is required to convert 77.6 g of solid iron at 21 °C to liquid iron at 1538 °C? The molar heat of fusion of iron is 13.8 kJ/mol. Iron has a normal melting point of 1538 °C. The specific heat capacity of solid iron is 0.449 J/(g · °C). q= kJ

From 25.0°C to 94.5°C, 75.1 grams of ethanol are heated. What was the energy requirement in joules?H(vap) 38.6 kJ/mol and H(fus) 4.60 kJ/mol are the heats of vaporization and fusion, respectively, for ethanol. cp (liquid) ethanol 2.46 J/g°C, cp (gas) ethanol 1.43 J/g°C, and cp (solid) ethanol 2.42 J/g°C are the specific temperatures for the three phases of ethanol. Ethanol has a molecular weight of 46. The melting point of ethanol is -114.1 °C and the boiling point is 78.4 °C.

Calculate the amount of heat (in kJ) required to raise the temperature of a 86.0 g sample of ethanol from 198.0 K to 300.0 K. The specific heat capacity of ethanol is 2.42 J/g°C. 60.0 kJ 21.2 kJ 11.9 kJ 75.6 kJ 28.4 kJ