huch heat is required to convert 125 g of bromine, Br2, from a solid to a liquid at its g point of -7.2 °C? The heat of vaporization of bromine is 193 J/g, the heat of fusion of he is 66.2 J/g and the specific heat of liquid bromine is 0.473 J/gºC

How much heat is required to convert 25g of ice at -6.0 ˚C to water vapor at 102 ˚C? (ΔHfus = 6.02kJ/mol; ΔHvap = 40.7kJ/mol ; specific heat of water is 4.184J/g●oC; specific heat of ice is 2.06J/g●oC; specific heat of water vapor is 2.03J/g●oC)

Consider the following selected properties of water: Density (liquid water): d = 1.00 g/mL Heat of fusion: AH fus Heat of vaporization: AHvap = 40.67 kJ/mol Specific heat (liquid water): cp = 4.184 J/(g∙K) = 4.184 J/(g•°C) = 6.8 kJ 380 J 68 kJ 3.8 kJ 75 J 6.01 kJ/mol How much heat is needed to heat 36 mL of water from 5 °C to 50 °C?

Butane is a common fuel used in cigarette lighters and camping stoves. Normally supplied in metal containers under pressure, the fuel exists as a mixture of liquid and gas, so high temperatures may cause the container to explode. At 25.0 ° C, the vapor pressure of butane is 2.30 atm. What is the pressure in the container at 130.0 ° C? ( Δ H °  vap = 24.3 kJ/mol.)

A particular refrigerator cools by evaporating liquefied dichlorodifluoromethane, CCl,F. How many kilograms of this liquid must be evaporated to freeze a tray of water at 0°C to ice at 0°C? The mass of the water is 549 g, the heat of fusion of ice is 6.01 kJ/mol, and the heat of vaporization of dichlorodifluoromethane is 17.4 kJ/mol. kg

Liquid ammonia can be used as a refrigerant and heat transfer fluid. How much energy is required to convert 25.0g of NH3(l) at -76 degrees Celsius into NH3(g)? In other words how much heat is needed to turn the liquid ammonia into a gas? molar mass: 17.03g/mol normal boiling point: -33.4 degrees Celsius  specific heat of NH3(l): 4.7 J/g . Degrees Celsius  specific heat of NH3(g): 2.2J/g . Degrees Celsius  molar heat of vaporization: 23.5 kj/mol

13. How much heat in kJ is needed to warm 31.6 g of ice from 10 °C to steam at 175 °C. The heat capacity of ice is 2.09 J/g °C, liquid water has a heat capacity of 4.18 J/g °C, and that of šteam is 1.84 J/g °C. The AHtus for water is 6.02 kJ/mol and the AHvap for water is 40.7 kJ/mol.

3. The enthalpy of fusion for Lauric acid (C12H24O2) is 32.86 kJ/mol and enthalpy of vaporization is 63.82 kJ/mol. The melting point is 43.2°C. How much heat is absorbed to raise the temperature of a 0.650g sample from 22.0°C to 56.3°C? The heat capacity of the solid is 2.15 J/g.C and the heat capacity of the liquid is 3.62 J/g°C.

79.2 grams of H2O is cooled from 115 °C to -43.1°C.  What is the heat change in joules?The molar heat of vaporization of H2O is 40.8 kJ/mol.  The molar heat of fusion of H2O is 6.02 kJ/mol.  Cp (solid) for H2O is 2.11 J/g°C.  Cp (liquid) for H2O is 4.18 J/g°C.  Cp (gas) for H2O is 2.00 J/g°C.  The melting point of H2O is 0.0 °C and the boiling point is 100.0 °C.

The heat of vaporization for ethanol is 0.826 kJ/g0.826 kJ/g. Calculate the heat energy in joules required to boil 20.65 g20.65 g of ethanol.