Class 9 Exam > Class 9 Notes > Science Class 9 > Theory - To Determine the Melting Point of Ice, Lab Experiment, Chemistry, Class 9 Science
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The Theory
CAN YOU DEFINE THE MELTING POINT OF A SOLID?
Melting point of a solid is defined as the temperature at which a solid changes into a liquid. Melting point of a solid indicates the strength of the force of attraction between the particles of the solid. On heating a solid, its molecules absorb energy in the form of heat and their kinetic energy increases.
As the kinetic energy increases, the temperature of the solid increases. As a result, the force of attraction between the molecules decreases and the molecules become more and more separated. This increases the potential energy of the molecule and the particles leave their fixed positions and start moving more freely.
At a particular temperature, the separation of the molecules increases by a large amount and the solid melts and converts into liquid. This particular temperature is the melting point of that solid. The melting point of a pure substance is always higher than the melting point of that substance when a small amount of an impurity is present. Pressure also affects the melting point of a substance. As the pressure on the substance increases, the melting point decreases.
WHAT ARE THE BENEFITS OF KNOWING THE MELTING POINT OF A COMPOUND?
The melting point of a compound helps in the identification of that compound. Measurement of the melting point of a solid can also provide information on the purity of the substance. Melting point of mixtures is lower than the melting point of a pure solid. Pure crystalline solids melt over a very narrow range of temperatures, whereas mixtures melt over a broad range of temperatures.
The temperature of the reverse change from liquid to solid is called the freezing point or crystallization point. For most substances the melting point and freezing points are equal.
For ice, the melting point is 0°C or 273K. The chemical element with the highest melting point is tungsten (3410°C), which is used for making filaments in light bulbs.
During the melting process, till all the ice melts, the temperature of the system does not increase until after the melting point is reached. The whole of the supplied heat energy is consumed in increasing the potential energy of the ice molecules. The kinetic energy of the molecule does not increase further, and the temperature does not increase, so long as the melting continues.
The quantity of heat required to completely change 1 kg of ice into water at atmospheric pressure at its melting point is called latent heat of fusion. For ice, it is 3.34 x 105 J/kg at 0°C.
Melting points of some common substances are given in the table.
Substance | Melting point (°C) |
Ice | 0 |
Mercury | ~-39 |
Hydrogen | -259 |
Oxygen | ~-219 |
Helium | ~-272 |
Glucose | 146 |
Iron | ~1535 |
Silver | ~961 |
Gold | 1063 |
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FAQs on Theory - To Determine the Melting Point of Ice, Lab Experiment, Chemistry, Class 9 Science - Science Class 9
| 1. How do you determine the melting point of ice in a lab experiment? |  |
Ans. To determine the melting point of ice in a lab experiment, you can follow these steps:
1. Take a beaker and fill it with crushed ice.
2. Place a thermometer into the beaker, ensuring that the bulb of the thermometer is submerged in the ice.
3. Heat the beaker slowly using a Bunsen burner or a hot plate.
4. Continuously stir the ice-water mixture to ensure even heating.
5. Observe the temperature on the thermometer as the ice starts to melt.
6. Note down the temperature when all the ice has melted. This is the melting point of ice.
| 2. Why is it important to use crushed ice instead of ice cubes in the experiment? | |
Ans. It is important to use crushed ice instead of ice cubes in the experiment because crushed ice has a larger surface area. This increased surface area allows for faster heat transfer, ensuring that the ice melts uniformly. Using ice cubes may result in uneven melting and inaccurate melting point measurements.
| 3. What is the melting point of ice? | |
Ans. The melting point of ice is the temperature at which solid ice changes phase and becomes a liquid. It is commonly known to be 0 degrees Celsius or 32 degrees Fahrenheit at standard atmospheric pressure. At this temperature, the ice absorbs enough heat energy to break its molecular bonds and transition into liquid water.
| 4. How does the melting point of ice change under different pressures? | |
Ans. The melting point of ice decreases as the pressure increases. This is because the application of pressure reduces the molecular motion and spacing in the solid ice, making it harder for the ice to maintain its solid state. As a result, the ice molecules require less thermal energy to break their bonds and transition into a liquid, causing the melting point to lower.
| 5. Can impurities affect the melting point of ice? | |
Ans. Yes, impurities can affect the melting point of ice. When impurities, such as dissolved salts or minerals, are present in the ice, they disrupt the regular arrangement of water molecules. This interference weakens the molecular bonds, making it easier for the ice to melt at a lower temperature than pure ice. Therefore, the presence of impurities leads to a decrease in the melting point of ice.
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