A 124.0 gram sample of an unknown substance (MM = 189.50 g/mol) is cooled from 233.0 \deg C to 147.6 \deg C. ( heat capacity of liquid = 1.62 J/g. \deg C; heat capacity of gas = 1.04 J/g. \deg C; AHvap = 78.11 kJ/mol; normal boiling point, Tb = 160.3 \deg C) How much energy (in kJ) is absorbed/released to condense the gas?

H8. The enthalpy of vaporization of benzene, C6H6(l) is 33.9 kJ/mol at 298 K. How many liters of C6H6(g), measured at 298 K and 95.1 mm Hg are formed when 1540 J is absorbed by, C6H6(l) at a constant temperature of 298 K? (Anwser in L) How do you work this problem out correctly using Clausius-Clapeyron Equation?

The heat absorbed or liberated by a substance (q) can be calculated using the following equation: q = g C ΔT, where g is the mass in grams, C is the heat capacity per unit mass, and ΔT is the change in temperature. Use the following values to calculate the energy required to convert one gram of ice at 0°C to one gram of steam at 100°C. The heat capacity of water is 4.25 J/g °C. The heat of fusion (the amount of heat required to change a solid into a liquid at its melting point) of ice is 335 J/g. The heat of vaporization of water is 2258 J/g.

Calculate the amount of heat (in kilojoules) required to vaporize 2.24 kgkg of water at its boiling point. (ΔHvap=40.7 kJ/molΔHvap=40.7 kJ/mol at 100∘C.∘C.)Express your answer to three significant figures and include the appropriate units.