When the system is heated, energy is transferred into it. In response to the energy it receives, the system changes, for example by increasing its temperature. A plot of the temperature versus time is called the heating curve. One such heating curve is shown here.
When a system contains only one phase (solid, liquid or gas), the temperature will increase when it receives energy. The rate of temperature increase will be dependent on the heat capacity of the phase in the system. When the heat capacity is large, the temperature increases slowly, because much energy is required to increase its temperature by one degree. Thus, the slope of temperature increase for the solid, liquid, and gases are different.
For example, the temperature of a system containing ice below its melting point will increase when heated. However, at 273.15 K, the temperature stops rising. At this temperature, the ice start to melt, and the heat is used to melt the ice. The melting of ice is called a phase transition. When energy supplied is used for the phase transition the temperature stays constant. After the phase transition is complete, the temperature rise will follow a different rate than that of the solid due to different heat capacity, as shown in the heating curve. A colorful web site for dicussing States of Matter also shows the heating curve, and phase diagram of water.
For one mole of water (18 g), we have the following data:
Water is a common substance. Ice is the stable phase below 273.15 K. Both solids and liquids coexist at 273.15 K. When heat is put into the system, more solid will melt. Thus, the temperature does not change. The normal boiling point is 373.15 K. As heat is absorbed, some water will boil off but the temperature is kept at 373.15 K. The changes in temperature as a function of time, or as a function of heat absorbed.
For water, the heat of fusion is 6.0 kJ / mol, and that of vaporization is 40.7 kJ/mol. If the heat input is constant, a longer period is needed for one mole of water to evaporate than the time needed for the ice to melt.
In a laboratory, we heat up different materials and plot the temperature as a function of time. Every material has a unique melting point and boiling point. It also has its heat of fusion and heat of vaporization.
Describe the melting point.
The experimental value is 6.01 kJ/mol which is equivalent to 80 cal/g. Which portion on the heating curve will be affected by the heat of fusion?
From the value given above, the heat capacity for water is larger than that of solid or gas. Heat capacity for gas H2O varies with temperature.
More energy is required to separate water molecules due to strong hydrogen bonding. Only weak hydrogen bonding is present in ether. Heats of vaporization for water and ether are 40.67 and 26.0 kJ/mol respectively.
Gold atoms have more electrons around them. Boiling points: Cu, 2868 K; Au, 2933 K.
Heat of vaporization: Cu, 304 kJ/mol; Au, 310 kJ/mol.
40 * 9 / 6 = 60 kJ (Note units are not kJ/mol)
The units for the values may cause confusion.