How much heat is released when 105 g of steam at 100.0 C is cooled to ice at -­15.0 C? The enthalpy of vaporization of water is 40.67 kj/mol, the enthalpy of fusion for water is 6.01 kj/mol, the specific heat capacity of liquid water is 4.18 J/g C and the specific heat capacity of ice is 2.02 J/g C. (q heating = m x C x ΔT, q phase change = ΔH vap x n)

The chlorofluorocarbon C2Cl3F3 has a normal boiling point of 47.6 ºC.  The specific heats of liquid C2Cl3F3 and gaseous C2Cl3F3 are, respectively, are 0.91 J/g-K and 0.67 J/g-K.  The molar heat of vaporization of C2Cl3F3 is 27.49 kJ/mol.  Consider a 50.0 g sample of the liquid CFC at 5.0 ºC.  How much heat is required to form gaseous C2Cl3F3 at 80.0 ºC?     Question 11 options:   A)  8.19 kJ   B)  1454 kJ   C)  30.51 kJ   D)  3031 kJ   E)  10.36 kJ

How much heat (in kJ) must be added to change 11.6 g of H2O(s) at -8°C to steam at 110°C? The specific heat of H2O(s) is 2.09 J/g°C, of H2O(l) is 4.184 J/g°C, and of H2O(g) is 1.84 J/g°C. The heat of fusion of water is 334. 7 J/g and the heat of vaporization is 2259.4 J/g.

How much heat energy is required to convert 39.6 g of solid ethanol at -114.5 °C to gaseous ethanol at 147.2 °C? The molar heat of fusion of ethanol is 4.60 kJ/mol, and its molar heat of vaporization is 38.56 kJ/mol. Ethanol has a normal melting point of −114.5 °C and a normal boiling point of 78.4 °C. The specific heat capacity of liquid ethanol is 2.45 J/g. °C, and that of gaseous ethanol is 1.43 J/g. °C. q= 4326.84 kJ