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need lab preformed and lab report. i have attached all information needed. Including a detailed sample lab report, which is exactly how the final report should look.
– 1 –
Augusta Technical College
PHYS 1110L – Online Lab 3: Latent Heat of Fusion & Specific Heat
Objectives:
The purpose of this laboratory activity is to investigate the latent heat of fusion, specific heat,
thermal energy and the temperature of water and various metal objects. Experimental values
obtained from real data will then be compared to the accepted values. We will also explore the
various forms of energy and energy transfer using simulation software.
Equipment:
• Real data for Latent Heat of Fusion and Specific Heat (experiment previously performed)
• Scientific Calculator
• PhET Energy Forms and Changes Simulation Software
Theory:
• Latent heat of fusion for water ( Lf ) is the thermal energy ( Qf ) needed to melt one gram of
ice into water at temperature of zero degree Celsius (see below table for list of
accepted values):
𝑳𝒇 = 𝑸𝒇/𝒎 ⇒ 𝑸𝒇 = ±𝒎. 𝑳𝒇
Where: Lf = Latent heat of fusion, Qf = Thermal energy (heat), m = Mass of ice or water
• Specific heat of a metal object ( cmetal ) is the thermal energy ( QΔT ) that an object must absorb
or release to change its temperature ( ΔT ) by one degree Celsius (see below table for list of
accepted values):
𝒄𝒎𝒆𝒕𝒂𝒍 = 𝑸𝚫𝑻 /𝒎. 𝚫𝑻 ⇒ 𝑸𝚫𝑻 = 𝒄𝒎𝒆𝒕𝒂𝒍. 𝒎. 𝚫𝑻
Where: cmetal = Specific heat of metal, QΔT = Thermal energy (heat), m = Mass of metal,
ΔT = Temperature change of metal
• To determine the latent heat of fusion for water ( Lf ), we place ice in a calorimeter that contains
warm water. The ice starts at approximately 0 ºC, melts into water, and then warms up to the
same final temperature as the warm water. This thermal energy transferred to the ice is the same
as the thermal energy transferred from the initially warm water as it cooled down to the final
equilibrium temperature:
– 2 –
watericef
waterTiceTf
LostGain
LostGain
TcmTcmmL
Q
)()(
)( )(
|| ||
−=+
−=+
−=
=
ice
ificewater
wfwaterwater
f
m
)TT(mc)TT(mc
L
−−
−
−
=
Where: cwater = specific heat of water
mwater = mass of water
mice = mass of ice
Tw = initial temperature of warm water
Ti = initial temperature of ice ~ 0 oC
Tf = final equilibrium temperature of mixture
• To determine the specific heat of a metal ( cmetal ), we heat a metal and then place it in a
calorimeter that contains cool water. The metal starts at approximately 100 ºC, cools down, and
the cool water warms up to the same final equilibrium temperature. The thermal energy
transferred to the cool water is the same as the thermal energy transferred from the initially hot
metal as it cooled down to the final, equilibrium temperature:
metalwater
metalTwaterT
LostGain
LostGain
TcmTcm
)()(
)( )(
|| ||
−=
−=
−=
=
)(
)(
mfmetal
wfwaterwater
metal
TTm
TTmc
c
−−
−
=
Where: cwater = specific heat of water
mwater = mass of water
mmetal = mass of metal
Tw = initial temperature of cool water
Tm = initial temperature of hot metal ~ 100 oC
Tf = final equilibrium temperature of mixture
– 3 –
Part A – Latent Heat of Fusion:
• The experiment was previously performed, and the data was recorded using the above shown
apparatus setup for measuring the latent heat of fusion for water.
• Using a temperature sensor, the data collection program displayed the graph of Temperature
versus Time, as shown above.
• The calorimeter was half-filled with warm water of mass mwater, and few pieces of dried ice of
mass mice were added to the calorimeter while stirring the mixture. Mass values are recorded in
the below table.
• From graph of Temp versus Time, see above sketch, the values of the maximum (initial)
temperature of the warm water Tw and the minimum (final) temperature Tf were obtained and
recorded in the below table.
– 4 –
Part B – Specific Heat:
• The experiment was previously performed, and the data was recorded using the above shown
apparatus setup for measuring the specific heat of two metals.
• Using a temperature sensor, the data collection program displayed the graph of Temperature
versus Time, as shown above.
• A metal of mass mmetal was heated in in boiling water for at least 5 minutes (Tm ~ 100 oC ).
• The metal was then retrieved from the boiler, water on the metal was quickly shaken off, and
the metal was dropped it into the calorimeter that was half-filled with cool water of mass mwater.
Mass values are recorded in the below table.
• From graph of Temp versus Time, see above sketch, the values of the minimum (initial)
temperature of the cool water Tw and the maximum (final) equilibrium temperature Tf were
obtained and recorded in the below table.
– 5 –
Analysis:
• Part A – Latent Heat of Fusion:
1. The measured values of the various masses and temperatures are given in the below table.
2. Calculate the experimental latent heat of fusion for water (Lf ) using the equation in the theory
section and record the result in the below table.
3. Compare the experimental value to the accepted value given in the below tables by
calculating the % Error. Record value in the below table.
Percentage error is used to compare experimental (calculated) to accepted (true) values:
% Error = %100
||
−
A
EA
; Where: A = accepted value and E = experimental value.
4. How do the values compare and what factors do think may cause there to be a difference
between these values? Discuss
in your lab report.
5. Why do we dry the ice before dropping in the calorimeter?
Explain in your lab report.
6. Why did we not include the mass of the calorimeter (Styrofoam) in our calculations? Explain
in your lab report.
7. Derive in the theory section of your lab report the final equation for latent heat of fusion for
water (Lf ).
• Part B – Specific Heat:
1. The measured values of the various masses and temperatures are given in the below table.
2. Calculate the experimental specific heat of the two metals (cmetal) using the equation in the
theory section and record the results in the below table.
3. Compare the experimental values to the accepted values given in the below tables by
calculating the % Error. Record values in the below table.
Percentage error is used to compare experimental (calculated) to accepted (true) values:
% Error = %100
||
−
A
EA
; Where: A = accepted value and E = experimental value.
4. How do the values compare and what factors do think may cause there to be a difference
between these values? Discuss in your lab report
5. Why do we shake off any water on the metals before dropping them in the calorimeter?
Explain in your lab report.
– 6 –
6. Why did we not include the mass of the calorimeter (Styrofoam) in our calculations? Explain
in your lab report.
7. Derive in the theory section of your lab report the final equation for the specific heat of the
metals (cmetal).
Energy Forms and Changes Simulation:
• Explore the various types energy forms, phase changes, and temperature using the below PhET
Energy Forms and Changes Lab Simulation Software:
https://phet.colorado.edu/sims/html/energy-forms-and-changes/latest/energy-forms-and-
changes_en.html
Go to the “Intro” tab
> Drag 2 thermometers (upper left) to contact and measure the temperatures of the
“Iron cube” and “Water container”
> Drag “Iron cube” on top of a “Burner”
> Heat “Iron cube” by pulling up on burner temperature gauge and hold
> Observe thermometer temperature of cube increase
> Drag Iron cube and drop in “Water container”
> Observe two thermometer temperatures achieve equilibrium
> Repeat but now also heat/cool Water by dragging it on top of second burner
> Observe the effect on the two thermometer temperatures when they achieve equilibrium
> Repeat using “Brick cube” and/or “Olive Oil container”
> Observe the effect on the two thermometer temperatures achieve equilibrium
> Repeat by heating both Iron and Brick cubes on top of each other
> Observe thermometer temperatures of the two cubes increase
> Drag both cubes and drop in Water or Olive Oil container
> Observe the three thermometer temperatures achieve equilibrium
• Discuss observations and compare your lab and simulation results in your report conclusion.
• Save a screenshot (screen capture) of one trial of the energy forms and changes simulations to
include in the graphs section of your lab report
Lab Report:
• When writing the lab report, you must review and follow very carefully the Physics Lab Report
instructions and outline document.
• In your lab report, include the Title Page, Objectives, Theory, Equipment, Data, Graphs and
Screenshots, Calculations, Conclusions, Sources of Error, and References.
https://phet.colorado.edu/sims/html/energy-forms-and-changes/latest/energy-forms-and-changes_en.html
https://phet.colorado.edu/sims/html/energy-forms-and-changes/latest/energy-forms-and-changes_en.html
– 7 –
• Remember to show all equations and calculations in detail and to round the results to the correct
number significant digits and precision.
• In the conclusions section, be sure to summarize the final results, comment on the agreement
or disagreement of the results with the theory or expectations, answer analysis questions, and
discuss what you personally learned from this experiment and your observations/comments.
• Remember to also answer and discuss all analysis questions in your conclusions section.
• Submit your complete lab report electronically by the due date!
Tables of Accepted Values
Accepted Heat of Fusion Values
Substance cal/g kJ/kg
Water 79.5 333
Mercury 2.72 11.4
Hydrogen 13.9 58.0
Oxygen 3.32 13.9
Accepted Specific Heat Values
Substance cal/(g∙℃) J/(kg∙℃)
Zinc 0.092 390
Aluminum 0.21 900
Stainless Steel (Iron) 0.11 450
Copper 0.092 390
Brass 0.090 350
Ice 0.530 2220
Water 1.00 4187
Sea Water 0.93 3900
Styrofoam ~ 0.00 ~ 0.00
– 8 –
Physics – Online Lab: Latent Heat of Fusion and Specific Heat
Tables of Data and Results
• Part A – Latent Heat of Fusion:
Quantity Trial # 1 Trial # 2
Mass of water: mwater 249.0 g 212.0 g
Mass of ice: mice 52.0 g 16.0 g
Specific heat of water: cwater 1.00 cal/g∙℃ 1.00 cal/g∙℃
Initial temperature of warm water: Tw 28.4 °C 36.3 °C
Initial temperature of ice: Ti 0.00 ̊C 0.00 °C
Final equilibrium temperature of mixture: Tf 11.0 °C 28.5 °C
Accepted heat of fusion of water: Lf 79.5 cal/g 79.5 cal/g
Experimental heat of fusion of water: Lf (cal/g)
% Error
– 9 –
• Part B – Specific Heat:
Quantity Trial # 1 Trial # 2
Type of metal: Copper Brass
Mass of metal: mmetal 81.0 g 80.0 g
Mass of water: mwater 301.0 g 299.0 g
Specific heat of water: cwater 1.00 cal/g∙℃ 1.00 cal/g∙℃
Initial temperature of cool water: Tw 11.7 ̊C 15.0 ̊C
Initial temperature of hot metal: Tm 100.0 ̊C 100.0 ̊C
Final equilibrium temperature of mixture: Tf 13.9 ̊C 17.1 ̊C
Accepted Specific heat of metal: cmetal 0.092 cal/g∙C 0.090 cal/g∙C
Experimental Specific heat of metal: cmetal (cal/g∙C)
% Error
Grade = 10/10
V. Good!
Lab Partners: Ainsworth Kiffin & Sammir Condezo Gonzales
Online Lab 7 – Resistors in Series and Parallel
University Name
PHYS 1110 – 01
21 March 2021
Dr. Nader Copty
Objectives:
The objective of this activity is to investigate the relationship between the equivalent resistance
and individual resistors connected in series and parallel. We will also investigate the voltage
across and current through resistors connected in series and parallel using simulation software.
Theory:
Before starting the experiment, there are a few concepts and equations that need to be known in
order to perform the lab:
•A combination of resistors in a circuit can be replaced with an equivalent (total) resistor that
does not alter the circuit and has the same total current and potential difference as the actual
resistors.
•The relationship between the current, voltage, and resistance is given by Ohm’s law:
𝑽 = 𝑰𝑹
• Where:
o V = voltage or potential difference (V)
o I = current (A)
o R = resistance (Ω)
•Resistors connected in series have the same current flowing through them. The equivalent
(total) resistance, current, and voltage of series combination are given by:
• 𝑹𝑻 = 𝑹𝟏 + 𝑹𝟐 + 𝑹𝟑 +⋯
• 𝑰𝑻 = 𝑰𝟏 = 𝑰𝟐 = 𝑰𝟑 = ⋯
• 𝑽𝑻 = 𝑽𝟏 + 𝑽𝟐 + 𝑽𝟑 +⋯
•Resistors connected in parallel have the same voltage applied across them. The equivalent
(total) resistance, current, and voltage of parallel combination are given by:
•
𝟏
𝑹𝑻
=
𝟏
𝑹𝟏
+
𝟏
𝑹𝟐
+
𝟏
𝑹𝟑
+⋯
• 𝑰𝑻 = 𝑰𝟏 = 𝑰𝟐 = 𝑰𝟑 = ⋯
• 𝑽𝑻 = 𝑽𝟏 + 𝑽𝟐 + 𝑽𝟑 +⋯
•In this activity, we will simulate three resistors in various combinations in a circuit. We will
measure the current through the resistors, and the voltage cross the resistors.
•We will determine the experimental value of the equivalent resistance (RT Exp) using Ohm’s
law and the accepted value of the equivalent resistance (RT Acc) using the given equations.
Equipment and Materials:
• Computer
• Scientific Calculator
• PhET Circuit Construction Kit: DC – Virtual Lab Simulation
https://en.wikipedia.org/wiki/Graphing_calculator
https://creativecommons.org/licenses/by-sa/3.0/
Data:
• Part A- Resistor in Series
Trial 1: R1 = 15.0 Ω, R2 = 33.0 Ω, R3 = 100.0 Ω
Voltmeter & Ammeter
Across:
V (Volts) I (Amps)
R1 V1 = 12.2 V I1
= 0.81 A
R2 V2 = 26.8 V I2 = 0.81 A
R3 V3 = 81.1 V I3 = 0.81 A
Battery VT Acc
= 120.0 V IT Acc
= 0.81 A
Trial 2:
R1 = 100.0 Ω, R2 = 15.0 Ω, R3 = 33.0 Ω
Voltmeter & Ammeter
Across:
V (Volts) I (Amps)
R1 V1 = 81.1 V I1 = 0.81 A
R2 V2 = 12.2 V I2 = 0.81 A
R3 V3 = 26.8 V I3 = 0.81 A
Battery VT Acc
= 120.0 V IT Acc
= 0.81
• Part B- Resistor in Parallel
Trial 1: R1 = 15.0 Ω, R2 = 33.0 Ω, R3 = 100.0 Ω
Voltmeter & Ammeter
Across:
V (Volts) I (Amps)
R1 V1 = 120.0 V I1 = 8.00 A
R2 V2 = 120.0 V I2 = 3.64 A
R3 V3 = 120.0 V I3 = 1.20 A
Battery VT Acc
= 120.0 V IT Acc
= 12.8 A
Trial 2: R1 = 100.0 Ω, R2 = 15.0 Ω, R3 = 33.0 Ω
Voltmeter & Ammeter
Across:
V (Volts) I (Amps)
R1 V1 = 120.0 V I1 = 1.20 A
R2 V2 = 120.0 V I2 = 8.00 A
R3 V3 = 120.0 V I3 = 3.64 A
Battery VT Acc
= 120.0 V IT Acc
= 12.8 A
Graphs:
Part A
Trial 1 Trial 2
Part B
Trial 1 Trial 2
Calculations:
Part A
Trial 1:
R1 = 15.0 Ω R2 = 33.0 Ω R3 = 100.0 Ω
VT Exp = V1 + V2 + V3
= 12.2 + 26.8 + 81.1
= 120.1 V
% Error = ( (120 V – 120.1 V) / 120 V ) x 100% = 0.08%
IT Exp = (I1 + I2 + I3) / 3
= (0.81 + 0.81 + 0.81) / 3
= 0.81 A
% Error = ( (0.81 A – 0.81 A) / 0.81 A ) x 100% = 0.00%
RT Acc = R1 + R2 + R3
= 15.0 + 33.0 + 100.0
= 148 Ω
RT Exp = (VT Exp) / (IT Exp)
= (120.1 V) / (0.81 A)
= 148 Ω
% Error = ( (148 Ω – 148 Ω) / 148 Ω ) x 100% = 0.00%
Trial 2:
R1 = 100.0 Ω, R2 = 15.0 Ω, R3 = 33.0 Ω
VT Exp = V1 + V2 + V3
= 81.1 + 12.2 + 26.8
= 120.1 V
% Error = ( (120 V – 120.1 V) / 120 V ) x 100% = 0.08%
IT Exp = (I1 + I2 + I3) / 3
= (0.81 + 0.81 + 0.81) / 3
= 0.81 A
% Error = ( (0.81 A – 0.81 A) / 0.81 A ) x 100% = 0.00%
RT Acc = R1 + R2 + R3
= 100.0 + 15.0 + 33.0
= 148 Ω
RT Exp = (VT Exp) / (IT Exp)
= (120.1 V) / (0.81 A)
= 148 Ω
% Error = ( (148 Ω – 148 Ω) / 148 Ω ) x 100% = 0.00%
Part B
Trial 1:
R1 = 15.0 Ω R2 = 33.0 Ω R3 = 100.0 Ω
VT Exp = (V1 + V2 + V3) / 3
= (120.0 + 120.0 + 120.0) / 3
= 120.0 V
% Error = ( (120 V – 120 V) / 120 V ) x 100% = 0.00%
IT Exp = I1 + I2 + I3
= 8.00 + 3.64 + 1.20
= 12.8 A
% Error = ( (12.8 A – 12.8 A) / 12.8 A ) x 100% = 0.00%
RT Acc = 1 / (1/R1 + 1/R2 + 1/R3)
= 1 / ( (1/15.0) + (1/33.0) + (1/100.0))
= 9.35 Ω
RT Exp = (VT Exp) / (IT Exp)
= 120 V / 12.8 A
= 9.38 Ω
% Error = ( (9.35 Ω – 9.38 Ω) / 9.35 Ω ) x 100% = 0.32%
Trial 2:
R1 = 100.0 Ω, R2 = 15.0 Ω, R3 = 33.0 Ω
VT Exp = (V1 + V2 + V3) / 3
= (120.0 + 120.0 + 120.0) / 3
= 120.0 V
% Error = ( (120 V – 120 V) / 120 V ) x 100% = 0.00%
IT Exp = I1 + I2 + I3
= 1.20 + 8.00 + 3.64
= 12.8 A
% Error = ( (12.8 A – 12.8 A) / 12.8 A ) x 100% = 0.00%
RT Acc = 1 / (1/R1 + 1/R2 + 1/R3)
= 1 / ( (1/100.0) + (1/15.0) + (1/33.0))
= 9.35 Ω
RT Exp = (VT Exp) / (IT Exp)
= 120 V / 12.8 A
= 9.38 Ω
% Error = ( (9.35 Ω – 9.38 Ω) / 9.35 Ω ) x 100% = 0.32%
Conclusions:
In Trial 1 of Part A, the total experiment voltage was 120.1 V. This resulted in a 0.08% error.
The total experimental current was calculated to be 0.81 A with a 0.00% error. The accepted
value of the total resistance was 148 Ω, which I successfully calculated with a 0.00% error. For
trial 2 we yielded the same results despite the same placement of each resistor. We yielded a
voltage of 120.1 V, an experimental current of 0.81 A and the total resistance of 148 Ω.
In Trial 1 of Part B, the total experiment voltage was 120.0 V. This resulted in a 0.00% error.
The total experimental current was calculated to be 12.8 A with a 0.00% error. The total
accepted resistance was calculated to be 9.35 Ω while the total experimental resistance was
calculated to be 9.38 Ω, which I successfully calculated with a 0.32% error. For both trials we
yielded the same results despite the same placement of each resistor. So I conclude that the
position of the resistor doesn’t have any effect on the results as long as the values are the same in
each trial.
The final results obtained from the simulation do agree with the theory of this lab. The theory
stated that through Ohm’s Law voltage, the current is directly proportional to the voltage, and
inversely proportional to the resistance. When calculating our percent error for current and
resistance, it remained low, ranging from 0% – 2.21%. The low percent proved that the experiment
was accurate and precise. The placement and order of resistors has a great effect overall on all
parts of the experiment. Because they control the control of energy, similar to a dam, the remaining
electricity that can move throughout the system differs. This also depends on the strength of each
resistor.
Sources of Error:
The sources of error in this experiment maybe from:
• Inaccurate measurements of the voltmeter and ammeter.
• The quality of wires could greatly affect the measured conductivity.
• The uneven placement of the battery and resistors can also have an effect on the readings.
• The battery’s output would affect the proper voltage to perform the lab.
References.
• Copty, Nader. “Online Lab Experiment: Electric Charges and Fields” Handout. Online
• Walker, Jearl, Robert Resnick, and David Halliday. Halliday & Resnick Fundamentals of
Physics. 11th ed. Hoboken, NJ: Wiley, 2018. Print.
• https://phet.colorado.edu/sims/html/circuit-construction-kit-dc-virtual-lab/latest/circuit-
construction-kit-dc-virtual-lab_en.html
Contributions:
Ainsworth Kiffin:
• Title Page
• Objective
• Theory Part A
• Equipment
• Part A: Data, Calculations and Graphs
• Part A: Analysis
Sammir Condezo Gonzales:
• Theory Part B
• Part B: Data, Calculations and Graphs
• Part B: Analysis
• Part A and B- Analysis
• Sources of Error
• References
