PHSC 100 BSU Fluid Mechanics Thermal Energy and Thermodynamics Lab Report see the attached file for the experiment one is on transfer of thermal energy and

PHSC 100 BSU Fluid Mechanics Thermal Energy and Thermodynamics Lab Report see the attached file for the experiment one is on transfer of thermal energy and the other is heat loss and change in temperature . Physical Science (PHSC 100) Virtual Lab Expt. # 4: Transfer of
Thermal Energy
Name: ________________________ Section: _______ Date: ______
Note on this Virtual Lab Experiment
Read the introductory principle, procedures and experimental materials outlined below,
and understand as to how this virtual experiment would be conducted under real lab
condition to generate the theoretical data supplied under each procedural steps below.
After clearly understanding the procedure and the formula for the calculations, complete
the blank dotted lines by inserting the required calculation results, write brief discussions
on blank spaces provided as per the guideline, and Submit completed assignment back
in the Drop Box.
Introduction
If a cup of cold water is mixed with a cup of hot water, the final temperature of the
mixture will be between the two initial temperatures. Using information on the
temperature and volume of the hot and the cold water, the final temperature of the
mixture could be predicted. This virtual experiment involves mixing of equal volume
of cold and hot water and prediction of the final temperature of the mixture.
Objective:
To predict the final temperature of a mixture of cold and hot water of different
temperature
Required Equipment and Supplies
a) Styrofoam cups (small and large)
c) Electric stove
b) Thermometers (Celsius)
d) boiling pan or pot
Procedure
Step 1
To get equal volume of cold and hot water, first three small Styrofoam cups are marked
equally at about the three-quarter level. You can do this by pouring water from one cup to
the next and mark the level along the inside of each cup. This is to make the volume of
water equal in all cases.
Step 2
About a liter of water is brought to boiling in the boiling pan. The first cup is filled to the
mark with cold water from the tap. Then the second cup is filled with hot water from the
pan to the same level, using a beaker or a larger Styrofoam cup for scooping. The
temperature of both cups of water is measured in thermometer, and recorded in the blank
space a) and b) below.
a)
b)
Temperature of cold water = 200C_____
Temperature of hot water = 820C______
Step 3
Predicting the temperature of the water, when the two cups of different temperatures
indicated above, are mixed. The two cups of water are poured into the larger Styrofoam,
and the mixture is stirred slightly, and the temperature is measured and recorded (actual
measured temperature value is given on b) below. Calculate the predicted value and enter
it in the blank space below [on a)]. Note that the volume of both cold and hot water
are equal.
a)
Predicted or calculated temperature = ______________ (show calculation)
b)
Actual or measured temperature = 460C
If there is a difference between the calculated predicted value and the actual measured
value, what may have caused it, if there is a difference? State it in the blank lines below.
————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————————
The mixture water is discarded into the sink and the following experiment is continued.
Step 4
One smaller cup is filled to its mark with cold water from the tap. Another two
small cups are filled to their mark with hot water. The temperature of water in each
cup is measured and recorded [shown on a), b), and c)] below.
Predicting the temperature of the water when the three cups are mixed. The three
cups of water are poured into the larger Styrofoam cup, the mixture stirred slightly,
and its temperature recorded [actual temperature value for the mixture is given on e)]
below. Calculate and enter the predicted temperature value of the mixture and enter it
in the blank space of d.
Note that the volume of water in all three cups are equal
a)
Temperature of cold water: 200C
b)
Temperature of hot water (cup 1): 820C_______________
Temperature of hot water (cup 2): 830C_______________
c)
d)
e)
Predicted or calculated temperature of mixture: _______________ (show
calculation)
Actual temperature: 550C
How is the actual temperature of the mixture compared with the calculated and predicted
temperature value? If there is a difference, give possible explanations as to what might
have caused it in the following blank space.
——————————————————————————————————————————————————————————————————————————————————–Which of the water samples (cold or hot) changed more from the initial temperature,
when it becomes part of the mixture? In terms of energy conservation, suggest a reason
for why this happened.
———————————————————————————————————————————————————————————————————————————————————Step5
Two small cups are filled to their marks with cold water from the tap. The third cup is
filled to its marks with hot water. The temperature of each was measured and recorded
(a, b, c). Then the three cups of water are poured into the large Styrofoam cup, the
mixture stirred slightly, and the temperature recorded (e). Calculate and predict the
temperature of the mixture when the three cups of different temperature values given
below are mixed and enter it in the blank line of (d).
a) Temperature of cold water (cup 1): 190C
b) Temperature of cold water (cup 2): 210C
c) Temperature of hot water: 850C
d) Predicted or calculated temperature of mixture ——————— (show
calculation)
e) Actual temperature: 400C
How is the observed or actual temperature value (e) compared with the predicted or
calculated temperature value (d)? Give a possible explanation if there is a difference.
——————————————————————————————————–
———————————————————————————————————————————————————–
Which of the water samples (cold or hot) changed more when it became part of the
mixture? Suggest a reason for why this happened.
————————————————————————————————————————————————————————————————————————————————————-What determines whether the equilibrium temperature of a mixture of two masses of
water will be closer to the initially cold or hot water?
————————————————————————————————————————————————————————————————————————————————————–
Physical Science (PHSC 100) Virtual Lab Expt. # 5: Heat Loss and
Change in Temperature
Name: ________________________ Section: _______ Date: ______
Note on this virtual experiment
Read the introductory principle, procedure and experimental materials outlined below,
and understand as to how this virtual experiment would be conducted under real lab
condition to generate the data supplied in Tables 1 below. After clearly understanding the
procedure and the formula for the calculations, complete the blank columns with
calculated data, write brief discussions as per the guideline, and Submit it back in the
Drop Box.
Introduction
Heat always flows from objects of high temperature to those of low temperature, until the
temperature reaches equilibrium. If hot water is left at room temperature it will lose heat
until the temperature reaches its surroundings. The amount of heat lost (Q) is
proportional to the mass and specific heat capacity of the material and the change in
temperature. This can be determined using the following equation:
Q = mcΔT
Where Q is the quantity of heat lost in calories, m is the mass (in gram, 1 ml = 1g for
water), c is the specific heat capacity (1.0 cal/g 0C for water) and ΔT is the change in
temperature in Celsius.
The objective of this experiment is to study the quantity of heat lost and the change in
temperature of hot water under covered and uncovered conditions.
Materials Required
• Hot plate
• cardboard covers with holes
• Beaker
• Styrofoam cups
• Thermometer
• Graduated cylinder
• Stopwatch
Procedure
Heat Loss and Change in Temperature
A litter of water is brought to boiling in a pan on an electric hotplate.
100 ml of hot water is poured into cup #1 and another 100ml of hot water into cup #2
and the temperatures measured with separate thermometers.
Cup # 1 is left uncovered and cover cup #2 is covered with a piece of cardboard with a
hole in the center for inserting a thermometer. The thermometers are left to stay in
both covered and uncovered cups for continuous temperature measurement.
The initial temperature for both covered and uncovered cups is measured and recorded
in the appropriate column on the data table for both covered and uncovered at 0
minute and from then on at 10-minnutes intervals for 40 minutes.
Data Calculation and Interpretation Assignment
First calculate the change in temperature (∆T) for each time interval always by
subtracting the temperature at each time interval from the initial temperature (temperature
at 0 min) and enter values in the change in temperature column. Do this for both covered
and uncovered cups. Then calculate the total quantity of heat (Q=mcT) and heat loss
(Q = mc∆T) in calories for each time interval for both covered and uncovered cups and
enter values in the appropriate column. Where Q = total quantity of heat, m = mass of
water (1 ml=1g), c= specific heat of water, which is 1cal./g/0C, and ∆T =change in
temperature in 0C. Calculate and fill out all blank columns.Table. 1. Heat Loss /
Heat Gain
Q = M.C.∆T
Q = quantity of heat,
M = mass of water (1 ml of water = 1g)
C = specific heat capacity of water (1cal/g/0C),
temperature
Time
(min
)
Uncovered Cup
∆ T = change in
Covered cup
Heat Ratio:
Total Quncovered
Total Qcovered
Temp
(T)
cup #1
(0C)
0
min
10
min
20
min
30
min
40
min
85
∆T
Tota (0C
l
)
Q(M Fro
CT)
m
(Cal. initi
)
al
—
Heat
loss
Q=
MC∆
T
(cal.)
cumu
lative
Temp.
(T)
cup
#2
0
( C)
—
85
52
66
45
55
39
47
34
41
Total
Q
(MC
T)
(Cal.
)
Fro
m
initi
al
Heat
loss
Q=
MC∆T
(cal.)
(cumul
ative)
—
—
∆T
(0C)
Discussion
In the lined space below, briefly describe your experimental results by comparing the
change in temperature (T) and total quantity of heat (Q) through time, for the covered
and uncovered cups. Also give possible explanations for the differences in the rate and
quantity of change in Q and T values under the two conditions (covered and uncovered).
What does the heat (Q) ratio, between the uncovered and covered cups, through time
indicate to you?
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