What amount of heat (in kJ) is required to convert 19.5 g of an unknown solid (MM = 83.21 g/mol) at -5.00 °C to a liquid at 52.3 °C? (specific heat capacity of solid = 2.39 J/g･°C; specific heat capacity of liquid = 1.58 J/g･°C; ∆Hfus = 3.72 kJ/mol; normal freezing point, Tf = 10.3°C)

How much heat, in J, is required to bring a mixture of 0.500 g liquid water and 0.500 g ice at 0 C to 10 C? Use 4.18 J/(g C) for the specific heat of the liquid and 334. J/g for the heat of fusion of ice. J

What amount of heat (in kJ) is required to convert 16.6 g of an unknown solid (MM = 67.44 g/mol) at -15.4 °C to a liquid at 42.7 °C? (specific heat capacity of solid = 1.95 J/g･°C; specific heat capacity of liquid = 1.18 J/g･°C; ∆Hfus = 5.72 kJ/mol; normal freezing point, Tf = 28.3°C)

What amount of heat (in kJ) is required to convert 25.8 g of an unknown liquid (MM = 83.21 g/mol) at 19.2 °C to a gas at 93.5 °C? (specific heat capacity of liquid = 1.58 J/g･°C; specific heat capacity of gas = 0.932 J/g･°C; ∆Hvap = 22.5 kJ/mol; normal boiling point, Tb = 57.3°C)

15) Liquid ammonia, NH3(1), was once used in home refrigerators as the heat transfer fluid. The specific heat capacity of the liquid is 4.7 J/gK and that of the vapor is 2.2 J/gK. The enthalpy of vaporization is 23.33 kJ/mol at the boiling point. If you heat 500 g of liquid ammonia from -40.0 °C to its boiling point of -33.3 °C, allow it to evaporate, and then continue warming to -5.0 °C, how much energy must you supply? (4) n O

Calculate the amount of energy in kilojoules needed to change 207 g of water ice at –10 °C to steam at 125 ° C. The following constants may be useful: Cm (ice) = 36.57 J mol-1 °C-1 • Cm (water) = 75.40 J mol-1 °C-1 Cm (steam) = 36.04 J mol-1 °C-1 Afus H = +6.01 kJ mol 1 Avap H = +40.67 kJ mol- -1

What amount of heat (in kJ) is required to convert 29.3 g of an unknown solid (MM = 67.44 g/mol) at -15.4 °C to a liquid at 42.7 °C? (heat capacity of solid = 1.95 J/g･°C; heat capacity of liquid = 1.18 J/g･°C; ∆Hfus = 5.72 kJ/mol; Tf = 28.3°C)

How much energy is needed to convert 1.99 g of ice at 0.00 °C to liquid water at 34.0 °C? Specific heat capacity (ice) = 2.10 J/g⋅°CSpecific heat capacity (liquid water) = 4.18 J/g⋅°CHeat of fusion = 333 J/g

Ethanol (C,H5OH) melts at -114°C. The enthalpy of fusion is 5.02 kJ/mol. The specific heats of solid and liquid ethanol are 0.97 J/g-K and 2.3 J/g-K, respectively. How much heat (k.J) is needed to convert 25.0 g of solid ethanol at -135°C to liquid ethanol at -50°C?

What amount of heat (in kJ) is required to convert 15.2 g of an unknown liquid (MM = 67.44 g/mol) at 43.5 °C to a gas at 128.2 °C? (specific heat capacity of liquid = 1.18 J/g･°C; specific heat capacity of gas = 0.792 J/g･°C; ∆Hvap = 30.1 kJ/mol; normal boiling point, Tb = 97.4°C)