ELECTRICAL EQUIVALENT FINAL COPY ADITYA CHANDEL
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Lab: Electrical equivalent of heat
Name: Aditya Chandel Group ID:
00
Date of experiment:
4/5/22
Date of Report Submission:
5/3/22
Course and Section number:
103A
Instructor’s Name:
Sheldon Fereira
Partner’s Names:
Bassma Rahman and Ravi Manne Symbols utilized and recorded for this lab are: θ and Δ and Σ
Introduction: Objectives:
-
Identify electrical equivalent of heat of the water -
Identify energy and heat units -
Identify values from voltage current, time and mass of substance
-
Form equivalent heat of water
-
Application of conservation of energy Theoretical Background:
Utilizing the law of conservation of energy, we know that the total amount of energy will always stay constant. We know this simply because energy cannot be created or destroyed. However, it can be transformed to different types of energy. Using a coil, the flow energy can be shown using the E=PT for the power multiplied by time in the system. This will allow us to find the power, the voltage, and current values required. P=IV. To get the total heat gained by the system which is Q, the respective masses and specific heats of aluminum and water need to be used.The equation used is Q=m
w
c
w
(T
f
-T
i
)+m
c
*c
c
(T
f
-T
i
). This will be utilized in J
e
=E/Q to calculate the electrical equivalent of heat. We have two different systems which are open and closed. These rules apply to isolated and closed systems but open systems can also have matter be a part of the processes involved. Experimental Procedure:
Experimental Variables: The experimental values that we are utilizing to conduct the electrical equivalent of head lab are: Specific heat of aluminum/cup (c
c
), specific heat of water (c
w
), mass of water (m
w
) mass of cup (m
c
), temperature final (T
f
), temperature initial (T
i
), heat (Q), current (A in amps), voltage (V in volts), flow of energy (E),
Experimental procedure:
1. First, make sure the voltmeter is connected to the terminals of the heating coil. Observe voltages differences on the voltmeter and then plug in the output of the DC power supply, ammeter, and heating coil into one single series. This will allow the water to heat and will allow for measurements of changes happening when it comes to voltage and current. 1. Take the mass of the inner calorimeter cup when it is completely empty then you can fill the water up to 250 mL with cold water. Take the mass with the inner cup with water inside. with cold 2. Measure the mass of the inner cup and water together and then place them in the calorimeter.
3. There is W.E 2.5g inscribed on the lid of the calorimeter taking this into account when attaining the final mass of water by multiplying it in calculations to the mass of the lid. 4. Place the lid on along with the stirror and heating coil on top of the calorimeter. Turn on the powder supply and adjust the voltage output until the ammeter reads 1.5.
5. Record the voltage and turn the power supply. Put the thermometer in water and record initial and final
temperatures. Put the lid on with the stirrer and heating coil atop the calorimeter and then turn on the power supply. 6. Make sure the power supply is turned on and put a timer so you can record the ammeter and voltmeter every two minutes while stirring the water.
7. Turn off the power supply and record the final time. Keep stirring until you get an accurate final reading temperature.
Results:
Experimental Data:
Variables:
Mass of empty inner cup of calorimeter m
c
= 58.56g
Mass of inner cup with water m
c
+m
w
+2.5(mass of lid)=306.67g
Effective mass of water m
w
=307.45-57.62=248.11g
Time t=540 seconds
Initial Temperature of water T
= 19.8 C
Final temperature of water T
f
=25.4
℃
Table 1:
Time
[second]
Voltage [V]
Current [A]
Time
[second]
Voltage [V]
Current [A]
0
6.5
1.5
300
6.6
1.7
30
6.5
1.5
330
6.6
1.7
60
6.5
1.6
360
6.6
1.7
90
6.5
1.6
390
6.6
1.7
120
6.5
1.6
420
6.6
1.7
150
6.5
1.6
450
6.7
1.7
180
6.5
1.7
480
6.7
1.7
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8.52. Use the molar volume to calculate each of the following at STP:
a) the number of moles of CO, in 4.00 L of CO2 gas
b) the volume, in liters, occupied by 0.420 mole of He gas
c) the volume, in liters, occupied by 6.40 g of 02 gas
d) the number of grams of Ne contained in 11.2 L of Ne gas
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Introduction
A fuel is burnt and as much of the energy released as possible is
transferred to water by heating.
Using the fact that 4.18 J of energy are required to raise 1 g of water
by 1 °C, the amount of energy given out by the fuel can be
calculated. This can then be converted to the amount of energy
given out per mole in order to calculate the enthalpy change of
combustion of the fuel.
Pre-lab questions
1
The water is contained in a metal can. Why is a metal can
used and not a glass beaker or other similar container?
Ethanol and propanol were chosen for this experiment as
they are members of a homologous series. Identify the
homologous series to which they belong and give the next
member of the series.
One of the biggest causes of error in this experiment is heat
loss. Does this lead to systematic or random errors? Suggest
how these errors could be decreased.
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gasoline produces 48.0 kJ/g and the density of gasoline is 0.737 g/cm. (1.00 gal = 3.785 L)
Energy =
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Questions 5
Available until 16 Mar at 14:30
Time limit 20 Minutes
Instructions
الكويز عبارة عن حل شيت والمعطيات لكافة الأفرع
25 ml of 1M HCI (ag) at 23.4°C was added to 25 ml of 1M NaOH at 23.4°C. The final temperature of the reaction
mixture was 29.7 C. Calculate A H, (KJ/mol). Density of each solution is 1.04 g/ml and Specific heat of water
=4.184 J/g.C
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Use the References to access important values if needed for this question.
A sample of solid silver is heated with an electrical coil. If 30.4 Joules of energy are added to a 12.1
gram sample and the final temperature is 35.6 °C, what is the initial temperature of the silver?
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AH
CO
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Potentially Useful Reference Information
Kw
= 0.114 x 10-14 at 0°C
Kw
= 0.465 x 1014 at 15°C
Kw
= 0.681 x 10-14
at 20°C
Kw
= 1.00 x 10-14 at 25°C
Kw
= 2.42 x 10-14 at 37°C
Kw
= 9.61 x 1014 at 60°C
Acid
Ka
HCI
1.3 x 106
H2SO4
1 x 103
HNO3
2.4 x 101
HSO4
1.2 x 10-2
H3PO4
7.5 x 103
A student measures the temperature of an NaOH solution to be 15
degrees C. The student then measures the pH of this NaOH solution
to be pH = 12.39.
H3CCOOH
1.8 x 10-5
%3D
H2CO3
4.3 x 10:7
H2PO4
6.2 x 10-8
Determine the molarity of this sodium hydroxide solution at 15°C.
Error analysis is not necessary, but report your answer with 2
HCO3
4.8 x 10-11
significant figures.
HPO,2
4.8 x 10-13
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Potentially Useful Reference Information
Kw = 0.114 x 10-14 at 0°C
Kw = 0.465 x 10:14 at 15°C
Kw
= 0.681 x 10-14 at 20°C
Kw
= 1.00 x 10-14 at 25°C
Kw
= 2.42 x 10-14 at 37°C
Kw = 9.61 x 10-14 at 60°C
Acid
Ka
HCI
1.3 x 106
H2SO4
1 x 103
HNO3
2.4 x 101
HSO4
1.2 x 10-2
H3PO4
7.5 x 103
H3CCOOH
1.8 x 10-5
H2CO3
4.3 x 10-7
At 37°C, a beaker of water has a pH of 7. Is this water basic, neutral, or
acidic?
H2PO4
6.2 x 10-8
O Neutral
HCO3
4.8 x 10-11
O Basic
HPO,2
4.8 x 10-13
O Acidic
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1. How would you prepare the following solutions?
2. How would you prepare 100 mL of a 6 M H₂SO4 solution, starting from a 18 N H₂SO4 solution?
Chemicals available
• KCL (solid); MW = 74.6
●
H₂SO4 (liquid); MW=98, concentration of stock solution: 18N
NaOH (solid); MW= 40
Acetic acid (liquid); MW = 60; Concentration of stock solution: 6 M
Sodium acetate (solid); MW = 82
Sodium dihydrogen phosphate monohydrate (solid); (NaH₂PO4 H₂O); MW = 138
Sodium monohydrogen phosphate (solid); (Na₂HPO4); MW = 142
●
a. 0.2 L of 0.25% NaCl
b. 200 mL of 0.15 M NaCl
●
●
●
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8.46. A scuba diver 60 ft below the ocean surface inhales 50.0 mL of compressed air from a
scuba tank at a pressure of 3.00 atm and a temperature of 8 C. What is the final pressure of air,
in atmospheres, in the lungs when the gas expands to 150.0 mL at a body temperature of 37 C,
if the amount of gas does not change?
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Imagine you were provided with: a stirrer, a thermometer, a plastic cup, a stand, a piece of plywood with holes in it, through which a thermometer and a stirrer can pass, a large measuring cylinder, some warm water, some cubes of ice, a clean rag.
Measure the temperature (θR) of the room. Transfer a known volume (V1) of warm water into the cup that can fill it to about two thirds of its capacity. Keeping the cup open, stir the warm water continuously until its temperature falls down to a value θ1 that is about 5 or 60C above θR. Dry some small blocks of ice with a clean rag and drop them into the warm water. Place the wooden or cardboard lid over the cup, with the stirrer and the thermometer in the holes in it. Stir the water continuously and put just enough small blocks of ice in it to make its final steady temperature θ2 to be about 5 to 60C bleow θR . Pour all the water into a measuring cylinder and measure its volume V2 . Estimate…
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product, include coefficient next to compound, Ex: 1S, or
2Ag2S. No spacing
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Kw
= 0.114 x 10-14 at 0°C
Kw = 0.465 x 10:14 at 15°C
%3D
Kw
= 0.681 x 10-14 at 20°C
Kw
= 1.00 x 1014 at 25°C
Kw = 2.42 x 10-14 at 37°C
Kw
= 9.61 x 10-14 at 60°C
Acid
Ka
HCI
1.3 x 106
H2SO4
1х 103
HNO3
2.4 x 101
HSO4
1.2 x 10-2
H3PO4
7.5 x 10-3
H3CCOOH
1.8 x 10-5
H2CO3
4.3 x 10-7
At 37°C, a beaker of water has a pH of 7. Is this water basic, neutral, or
H2PO4
6.2 x 10-8
acidic?
HCO3
4.8 x 10-11
Neutral
Basic
HPO,2
4.8 x 10-13
Acidic
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3) Please predict the structure of the following molecules with the information you are given
A) Formula: CH,0,
H NMR Spectra
molbase.com
molbase.com
10
PPM
c" NMR Spectra
molbase.com
molbase.com
200
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160
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PPM
220
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60
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Write a 2-3 paragraph summary on an advanced material.
Make sure to include the following:
Describe the chemistry (i.e., molecular formula or chemical composition
1)
2) How is it currently produced
3)
What are its advantages/disadvantages to other materials that are used for the same purpose
Provide a reference for your information
4)
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Kw
= 0.114 x 10-14 at 0°C
Kw
= 0.465 x 1014 at 15°C
Kw = 0.681 x 10-14 at 20°C
%3D
Kw = 1.00 x 10-14 at 25°C
%3D
Kw = 2.42 x 10-14 at 37°C
Kw = 9.61 x 10-14 at 60°C
Acid
Ka
HCI
1.3 x 106
H2SO4
1х 103
HNO3
2.4 x 101
HSO4
1.2 x 10-2
A student measures the temperature of an NaOH solution to be 15
degrees C. The student then measures the pH of this NaOH solution
to be pH = 12.39.
H3PO4
7.5 x 103
H3CCOOH
1.8 x 10-5
In a separate experiment at 25°C, a student recorded that it took 25.8
mL of a 0.200M NAOH solution to completely neutralize 32.00 mL of
H2CO3
4.3 x 107
an unknown, diprotic acid solution. Determine the initial molarity of
H2PO4
6.2 x 10-8
this unknown acid solution.
Error analysis is not necessary, but report your answer with the correct
HCO3
4.8 x 10-11
number of significant figures.
HPO,2
4.8 x 10-13
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2. Two students are setting up a demonstration to show different ways that heat can be
transferred from a hot plate to a thermometer. They are provided with the
following materials: Beakers, Thermometers, Water, Sand, and Hot Plates. The
procedure is as follows.
1. Fill beaker #1 with water, and beaker #2 with sand.
2. Put a thermometer in the beaker with water and a thermometer in the beaker
with sand.
3. Record the temperature of the sand and the water.
What are the next steps and which description accurately represents the transfer of
heat?
A. Step 4: Place each beaker on a separate hot plate and tums on the hot plate.
Step 5: Record the temperature every minute.
Explanation: Beaker #1 demonstrates heat transfer by convection and beaker #2
demonstrates heat transfer by conduction.
B. Step 4: Place each beaker on the lab bench
Step 5: Record the temperature every hour.
Explanation: Both beakers demonstrate heat…
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The real gases do not follow the ideal gas law of PV= nRT, where P is the pressure, V is the
volume, n is the amount of gas, R is the Universal gas constant, and T is the absolute
temperature.
(a)
Identify the variables in the ideal gas that are responsive for the deviation and draw
their respective diagrams.
(b)
Explain the reasons for deviation of the behaviour of the real gases from the ideal gas
law.
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12:52 PM
30°C Light rain
A 4)) G DO
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Ac₂0/NaOAc
PhCO,H
HNO,/H₂SO4
Now
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C13 NMR Peaks
Aldehydes
RCO)R
Aldehydes and ketones
Carbaxylic
R(CO)X
Carbaxylic acid derivatives
Ntrile
Nitrile RCN
CC
C-C
Alkyne
Akyne R-CC-R
RCH20
RCH2-O
R4C
RAC
R3CH
R3CH
RCH2X
X= C-C, C-O, Br, CI, N
RCH2X
R2CH2
RECH2
RCH3
RCH3
TMS
TMS
220
200
180
160
140
120
100
80
60
40
20
Typical chemical shifts in 13c-NMR
9) Why do the peaks of associated with aldehydes (both in H NMR and C NMR) appear so much further
downfield than other peaks?
C13 NMR Peaks E
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MODULE 4: assign 1
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Can you please answer e,f,g, and q 2, thanks
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Absorbance (arb.units)
SA
8.3
B-Carotene Calibration Curve
2004
65,03UM
3.26 mM
5,06 nM
y=(105612 Mx-0.1736
2.94 M
4304 1064 ENY 181 121
Concentration (M)
1004
5
Abserbence (arb.units)
200
0.25
300
A student creates a standard curve of B-Carotene and plots the line of best fit. They then measure the
absorbance of a solution of B-Carotene with an unknown concentration. What is the concentration of
the sample? You can assume they used a cuvette with a pathlength of 1 cm.
400
500
600
Wavelength (nm)
YOU
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Question 1
1 pt
Question 2
2 pts
"Heater Meals" are food packages that contain their own heat source. Just pour water into the heater unit, wait a few minutes, and voilà! You have a hot meal.
Mg(s) + 2 H2O(l) → Mg(OH) 2 (s) + H2(g)
Question 3
1 pt
Species
AH° (kJ/mol) S° (J/mol·K) AƒG° (kJ/mol)
Question 4
2 pts
Mg(s)
0
32.67
0
Question 5
1 pt
Question 6
× 2 pts
H2O(l)
Mg(OH)2(s)
-285.83
69.95
-237.15
-924.54
63.18
-833.51
H2(g)
0
130.7
0
Question 7
1 pt
Question 8
2 pts
Question 9
1 pt
HEATER MEALS
Question 10
2 pts
Question 11
1 pt
Question 12
1 pt
Question 13
Charles D. Winters
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34 ou b
HEATER MEALS
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Question 14
1 pt
The heat for the heater unit is produced by the reaction of magne-
sium with water.…
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Theoretical Background
Sections related with heat transfer from thermochemistry topic will be discussed.
Experimental Procedure
Describe the experiment as you did it in your own words with in a paragraph.
Calculations
Show all your calculations here. For this experiment you need to give calculations about how you
calculated heat lost for water (Qwater) and heat gain by ice (Qice).
Conclusions
Describe what you learnt from the experiment and suggest improvements
Data Sheet
mice = 20 gram
Tice = 0 °C
maxater = 300 gram
Twater = 30 °C
Itinal = 22 °C
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25
1.
T
The specific heat of water is 4.18 J-g-¹ K-¹. How much heat is required to raise the temperature of 500 g of
water from 20 °C to the boiling point (100 °C)? What is the molar heat capacity of water?
Specific heat of 11₂0= 4₁185.5-1-14-1
motor mass of waver: 18,001g/mol
mas of water = 5003
a.
5
D
HRAMCAT
Hear = 500g (thit 3). 2014
Initial Temp: 20%= 2931
molar hear capacity & spresse head capacting of w
Anal Temp: 100% = 3731
Hear =?
Molar heat coperty?
Hent = 1672003
Hear = 167.23
= 4.182 * 75,23/10.19
2. In studying the energy generated by a person, you may view the person roughly as a constant pressure
calorimeter using sugar (i.e., sucrose, C12H22O11) to generate power. The reaction of table sugar in a
calorimeter is given by
C.
Q
b. Calculate the enthalpy of combustion per mole of sugar utilization.
Does the result of your calculation make sense?
C12H22O11(s)+120₂(g) →12CO₂(g)+11H₂O+heat.
→give the magnitudo (no sign is recessure)
What is the heat released by consuming one…
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I need step by step process solving [4.184x156(Tf-295)] + [4.184x85.2(Tf-368)] = 0. because my work is wrong. Thank you!!
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Part A
transcript When glucose (C6H12O6 (s)) is consumed, it reacts with O₂ gas in the body to produce gaseous carbon dioxide and liquid water. Enter the balanced chemical equation for the reaction.
Express your answer as a chemical equation including phases.
0
ΑΣΦ
?
A chemical reaction does not occur for this question.
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3. Consider the reaction: 2NO(g) + O2(g
NO2 is 33.8 kJ/mole, calculate AH°f for NO
AH=-113.1 kJ. If AH° for
(3)XONZ
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1. CH31 (excess)
2. Ag20, H2O, heat
NH2
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The average adult human burns 2.00 x 10° kcal per day in energy. What is this rate
in kJ per hour ?
STARTING AMOUNT
ADD FACTOR
ANSWER
RESET
*( )
1
4184
349
1000
0.001
1.15 x 105
4.184
60
2.00 x 10°
2.01 x 10°
24
20.0
J
cal
kJ
min
kcal/day
kcal
hr
9:26 PM
P Type here to search
a
A O G E D 4)
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5/4/2021
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4- Use Hess's law to calculate the enthalpy change (in kJ/mol) of Alanine oxidation (ΔH1) using the below individual steps.
C3H7NO2(s) + 3O2(g) → 5 2 CO2(g) + 5 2 H2O(l) +1 2 (H2N)C=O(s) ΔH1 =??
(H2N)C=O(s) + 3 2 O2(g)→CO2(g) + 2 H2O(l) + N2(g)
ΔH2 = -632 KJ/mol
C3H7NO2(s) + 15 4 O2(g) → 3 CO2(g) + 7 2 H2O(l) + 1 2 N2(g)
ΔH3 = -1577 KJ/mol
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if a volumetric pipet delivers 24.844g of deionized water at 31.00 degrees C, what is the calibrated volume of the pipet?
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us_engine.html?ClassID=1463972376#
The energy for the system to reach
20.5 °C is supplied by a chunk of hot
metal. What would be the initial
temperature of a 30.0 g piece of the
metal?
qmetal= -2113 J
Cmetal = 0.575 J/g°C
T₁ = [?] °C
Initial Temp (°C)
Enter
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Radioactive decay can be described by the following equation
In A = In Ao – kt
where Ao is the original amount of the substance, A is the amount of the substance remaining after time t, and k is a
constant that is characteristic of the substance.
-1
For the radioactive isotope iodine-123, k is 5.21 × 10-2 hours.
If the original amount of iodine-123 in a sample is 48.1 mg, how much iodine-123 remains after 13.2 hours have passed?
mg
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- Chemistry by OpenStax (2015-05-04)ChemistryISBN:9781938168390Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark BlaserPublisher:OpenStax
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