13. Liquids, Solids & Intermolecular Forces

How much energy (kJ) is required to convert a 76.4 g acetone (MM = 58.08 g/mol) as a liquid at -30°C to a solid at -115.0°C?

If 53.2kJ of heat are added to a 15.5g ice cube at - 5.00 ^oC, what will be the resulting state and temperature of the substance?

How much energy is released when 42.5 g of water freezes?

What quantity of heat, in kj, is required to convert 50.0 g of ethanol (C₂H₅OH) at 23.0°C to a vapor at 78.3°C (its boiling point)? (specific heat capacity of ethanol = 2.46 J/g • c; ∆H_vap = 39.3 kJ/mol)

Which is the process by which a gas changes to a solid: deposition, evaporation, freezing, or sublimation?

What are greenhouse gases? How does carbon dioxide enter the atmosphere? (Site 1)

If the heating curve is reversed, what would best describe the boiling point?

If 54.0 kJ of heat is gradually added to a 1.00 mol sample of liquid ethanol with an initial temperature of 298 K, the heating curve shown here is obtained. Use this graph to answer the following questions.

a. What is the boiling point?

b. What is the enthalpy of vaporization in kJ/mol?

c. Is the specific heat of liquid ethanol greater than or less than the specific heat of gaseous ethanol? [Section 11.4]