# A substance has the following properties: Heat capacities: 1.34 J/g oC (solid) 3.02 J/g oC (liquid) 2.55 J/g oC (gas) Heat of Fusion = 4.23 kJ/mole Heat of Vaporization = 23.5 kJ/mole Melting Point =

A substance has the following properties: Heat capacities: 1.34 J/g oC (solid) 3.02 J/g oC (liquid) 2.55 J/g oC (gas) Heat of Fusion = 4.23 kJ/mole Heat of Vaporization = 23.5 kJ/mole Melting Point = -30.0 oC Boiling Point = 88.5 oC Molar Mass = 33.4 g/mole How much energy (in kJ) would be needed to heat 50.0 g of this substance from -40.5 to 102oC? Enter the E1 – E5 energies and the total energy in the spaces below. Recall that E1 is the energy absorbed by the solid up to the final temperature or melting point (whichever is reached first) E2 is the energy absorbed when the solid is converted to a liquid E3 is the energy absorbed by the liquid up to the final temperature or boiling point (whichever is reached first) E4 is the energy absorbed when the liquid is converted to a gas E5 is the energy absorbed by the gas. One or more of the energies may be 0 kJ. …

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A substance has the following properties: Heat capacities: 1.34 J/g oC (solid) 3.02 J/g oC (liquid) 2.55 J/g oC (gas) Heat of Fusion = 4.23 kJ/mole Heat of Vaporization = 23.5 kJ/mole Melting Point =
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