experiment to show the effect of heat on ice with aim , observation, procedure, materials required,result, precaution.
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Answers
Experiment 4-Heat of Fusion and Melting Ice Experiment In this lab, the heat of fusion for water will be determined by monitoring the temperature changes while a known mass of ice melts in a cup of water. The experimentally determined value for heat of fusion will be compared with the accepted standard value. We will also explore the following question regarding the rates of melting for ice cubes is posed: Will ice cubes melt faster in distilled water or in salt water? Part A-Heat of FusionA phase change is a term physicists use for the conversion of matter from one of its forms (solid, liquid, gas) to another. Examples would be the melting of solid wax to a liquid, the evaporation of liquid water to water vapor, or condensation of a gas to a liquid. The melting of a solid to a liquid is called fusion. As a phase change occurs, say the evaporation of boiling water, the temperature of the material remains constant. Thus, a pot of boiling water on your stove remains at 100 °C until all of the water is gone. Even if the pot is over a big flame that is 900 °C, the water in the pot will only be 100 °C. A tray of water in your freezer will approach 0 °C and remain at that temperature until the water is frozen, no matter how cold the freezer is. In a phase change, heat energy is being absorbed or emitted without changing the temperature of the material. The amount of energy that is absorbed or emitted during a phase change obviously depends on the mass of the material undergoing the change. It takes more energy to melt a bag of ice than it takes to melt a single ice cube. The amount of energy also depends on the substance, because of the particular composition of each substance. It takes 80 calories of heat energy to melt 1 g of ice. This is the heat of fusion (Hfusion) for ice (heat required per gram of substance). In order to determine the heat of fusion for ice, we need to melt some ice and measure how much heat energy is absorbed. The ice needs to be isolated from its surroundings, so we place it in an insulating Styrofoam cup, which is a simple device called a calorimeter (heat measurer). Measuring changes in heat energy is simply measuring changes in temperatures. Warm water will be used in the Styrofoam cup to melt the ice. Recall that the mass of the ice is important. It is hard to weigh ice without melting some of it, so the mass of the ice will be determined after it has melted. As ice melts (at a constant temperature of 0 °C), it forms water at 0 °C, absorbing heat energy form the warm water. This cold water then needs to be warmed, which absorbs more heat energy form the warm water, until a final temperature is reached. The heat lost by the warm water must be equal to the heat gained by the ice and cold water. The property of specific heat (Hsp) is the amount of heat energy needed to change the temperature of one gram of a material by one degree Celsius. Like Hfusion, the value of Hsp depends on the substance. For example, it takes much more energy to heat up a pot full of water than it does to heat up the metal of the pot itself. Hsp for water is 1 calorie/ g °C.
The experiment to show the effect of heat on ice is to observe the change in state and temperature of the ice.
Explanation
EXPERIMENT TO SHOW THE EFFECT OF HEAT ON ICE -
AIM
To observe the effect of heat on ice.
MATERIAL REQUIRED
Beaker, thermometer, ice, flame.
PROCEDURE
- Take a beaker and fill it with the ice.
- Suspend the thermometer into the beaker so the bulb remains in contact with the ice.
- Note down the initial temperature of the beaker containing ice.
- Heat the beaker and let the ice melt.
- Observe the temperature change and note it down.
OBSERVATION
No change in temperature is observed with the change in state from solid to liquid on melting. As the provided heat gets absorbed in the particles during melting and does not lead to an increase in the temperature of the liquid.
RESULT
The heat causes the change in the state of ice from solid to liquid without the change in the temperature.
PRECAUTIONS -
- Carefully handle the beaker and wear gloves.
- Properly emerge the thermometer into the beaker.
- Note down the readings carefully to get accurate results.
- Observe the change in state and temperature carefully.