Ice Melting
(Fourth Laboratory Experiment)
Norada, Jessica H.
Vergara, Jelle R.
Gopo, Lee Anne
Partosa, Elton John G.
I.
INTRODUCTION
When temperature changes, matter can undergo a phase change. Phase change is
a process in which a substance shift from one phase to another. These changes
occur when sufficient energy is supplied to the system or sufficient amount is lost
and also occur when the pressure on the system is changed.
Melting (changing from a solid to a liquid), freezing (from liquid to a solid),
evaporation (from liquid to a gas), and condensation (from gas to a liquid) are
examples of phase change.
In this experiment, we will observe the temperature of glass of crushed ice. After
observing it, we will know what happens with the temperature of water while the
crushed ice was changing from solid to liquid.
II.
MATERIALS AND METHODS
i.
Materials
The following are the materials that are used for this experiment:
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ice
glass container/ beaker
thermometer
weighing scale
timer (stopwatch)
stirring rod (you can use other material as substitute for the stirring rod like spoon)
Figure 1. Materials used during the experiment
ii.
Methods
The following are the procedures for this experiment:
1. Get a piece of ice then weigh it.This will serve as your mass for 0
minute.
Figure 1.1 Cracked Ice
Figure 1.2 Weighing of the Ice
2. Ready the containers and then set it up with approximately 500mL of
cold water and measure its temperature. Let this be your temperature at 0
minute, and make sure that the temperature of the area is cold.
Figure 2.1 The 500ml of cold water was
poured into the pitcher
Figure 2.2 The temperature of the water was
measured
3. Fill in the container with ice and let it be mixed by stirring for 2 minutes.
After 2 minutes of stirring, measure the temperature of the water, and let it
serve as your temperature for 2 minutes.
Figure 3.2 The ice was stirred for 2 minutes
Figure 3. 1 The ice was put into the pitcher
Figure 3.3 The temperature was measured
after 2 minutes
4. After measuring, remove the ice and weigh the ice. Record its mass at 2
minute time.
Figure 5 The weight of the ice after 2 minutes is
0.90 g
5. Repeat the procedure 3-4 every 2 minutes for the 4,6,8 and 10 minutes.
Put the ice in the container and let it melt.
4 minutes
Figure 5.1. The water is stirred
together with the ice
Figure 5.2. The weight of the
ice after stirred
Figure 5.3. Measured
temperature of the water
6 minutes
Figure 5.4. The water is stirred
together with the ice
Figure 5.5. The weight of the
ice after stirred
Figure 5.6. Measured
temperature of the water
8 minutes
Figure 5.7. The water is stirred
together with the ice
Figure 5.8. The weight of the
ice after stirred
Figure 5.9. Measured
temperature of the water
10 minutes
Figure 5.10 The water is stirred
together with the ice
Figure 5.11 The weight of the
ice after stirred
Figure 5.12. Measured
temperature of the water
III.
RESULTS AND DISCUSSION
Phase changes are always goes along with change in the energy of a
system. As is the case, adding thermal energy by heat increases the
temperature of a substance. However, there are circumstances where
adding thermal energy does not change the temperature of a substance.
Instead, adding thermal energy acts to loosen bonds between molecules
that cause phase change (e.g. solid to liquid, liquid to solid, gas to liquid,
and liquid to gas).
In this activity, we used cold water and spoon to melt the ice (see Figure
1). The values for the mass, temperature, quantity of heat, and heat
current are shown in the table below.
Table 1 Mass, Temperature, Quantity of Heat, and Heat current of the ICE
Time (min)
Mass (g)
Temperature Quantity of Heat current
heat (J)
(J/sec)
(°C)
0 min
2 min
4 min
6 min
8 min
10 min
0.105 g
0.90 g
0.65 g
0.45 g
0.25 g
0.10 g
10°C
3°C
2°C
1°C
3°C
4°C
3.504𝑥10−4 J
3.006𝑥10−3 J
2.171𝑥10−3 J
1.503𝑥10−3 J
8.35𝑥10−4J
3.34𝑥10−4J
3.57𝑥10−4J
2.505𝑥10−5 J
9.046𝑥10−6 J
4.175𝑥10−6 J
1.739𝑥10−6 J
5.566𝑥10−7 J
In the time of 0 minute, the ice has mass of 0.105 grams with the
temperature of 10°C. 3.57𝑥10−4J heat transferred and 3.504𝑥10−4 J are
required energy to melt the ice (see Figure 3.1-3.3). After, the ice was
stirred for 2 minutes the weight of the ice is 0.90 grams with temperature
of 3°C. It has 2.505𝑥10−5 J heat transferred and 3.006𝑥10−3 J of energy
needed to melt the ice (see figure 5-5.1). The process was repeated for
the next 2 minutes wherein the mass of the ice gets lesser than the
previous results. The weight of the ice is 0.65 g and has temperature of
2°C where it takes 9.046𝑥10−6 J of heat transferred. 2.171𝑥10−3 J is the
required energy to melt the ice (see figure 5.1-3). The ice was stirred again
for the entire 2 minutes and it gets the mass of 0.45 grams (see figure 5.45). It has temperature of 1°C and takes 4.175𝑥10−6 J of heat energy,
while 1.503𝑥10−3 J of required energy needed to melt the ice (see figure
5.6).
In this process (see table 1; 0 minute to 6 minutes), we observed as the
mass is getting lesser the temperature decreases. Also, we noticed that
they are different from the values of heat transferred wherein for the 4
minutes it absorbs more heat energy than the 0 minutes, 2, 6, 8, and 10
minutes.
So, we consider that the ice is slowly melting through absorption of heat
energy. This transition is a more ordered to less ordered state and it is
called endothermic. The heat energy that the ice absorbs due to stirring it
breaks the bonds of bonds of the particles. Therefore, there is no rise in
temperature.
However, for the 8 and 10 minutes (see table 1), as the mass is still getting
lesser, the temperature increases. As you can see, the ice was stirred in 8
minutes has the lowest value of heat energy transferred among the rest
but has the higher required energy to melt the ice. It indicates that the
energy for a phase change is enormous compared to energy associated
with temperature changes. The heat transferred to the ice goes partly
toward the phase change (melting), and partly toward the raising
temperature after melting.
Figure 6. The remaining ice
was melted
Figure 6.1. The remaining ice
melted
Figure 6.2. The Ice melted
within 2:28.08 minutes
Figure 6.3. The measured
temperature of the water after
the ice melted
The ice is completely melted in 2 minutes and 28.8 seconds with the temperature of
5°C. In this phase, we observed that the temperature still increase even
though the ice is melted. When the ice was stirred in 0-6 minutes, the
temperature of the water is lower than the temperature of the water in 8-10
minutes. As the ice was slowly melting the mass is getting smaller until it’s
gone. The ice transformed into liquid at the melting temperature; then the
temperature of water rises. Hence, at lower temperature most substances
are solid; as the temperature increases, it becomes liquid.
The quantity of heat and heat current can be measured using the equation below:
IV.
Conclusion
Based on the conducted experiment we have observed that heat transfer was
evident on in the experiment. The capability of the piece of ice to change the
temperature of the water is concept of heat transfer. We also observed that phase
change was visible as we go along the experiment and through the passage of time.
As time passed by and we stir the ice on the water, the time and force affects the
mass of the ice and phase change was occurring. Therefore, we can conclude that
ice has a lower temperature and the surroundings have a higher temperature. So,
the system that is ice starts to absorb heat from the surroundings spontaneously and
starts to melt. This phenomenon is best described using the second law of
thermodynamics even without the usage of water. It will never happen for the ice to
lose heat and get even colder because it will violate the Second Law of
Thermodynamics.
V.
Recommendation
Based on the experiment we conducted, our best recommendation is to add different
substance on the experiment such as salt and sugar. We also recommend that the
experiment would be much better if not only ice melting was performed but also
experiments for phase changes, like sublimation, evaporation and condensation so
that you'll have a better understanding and an actual presentation on how do these
processes work.
VI.
Reference
 https://chem.libretexts.org/Bookshelves/General_Chemistry/M
ap%3A_General_Chemistry_(Petrucci_et_al.)/12%3A_Intermole
cular_Forces%3A_Liquids_And_Solids/12.4%3A_Phase_Diagr
ams
 https://openstax.org/books/physics/pages/11-3-phase-changeand-latent-heat
 https://opentextbc.ca/introductorychemistry/chapter/phasetransitions-melting-boiling-and-subliming/