CHEM1B - Calorimetry Lab Report Template (1)
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EVC - CHEM1B
Name: Whitney Bourassa
Name(s) of Lab Partners: Quinn, Nugene
Date: 2/13/24
Calorimetry Lab Report
OBJECTIVE(S): METHODS:
The procedures for this experiment were taken from lab manual: Valentin, J. et al, General Chemistry II (Chemistry 1 B) Experiments. (2020 Version). Evergreen Valley College, San Jose, CA.
DATA:
Part B: Calibration of Calorimeter.
Calorimeter number = 11
Data for Experiment:
Part B #1
Time (s)
Temp 0
21
30
29.5
60
29.5
90
29
120
29
150
29
180
28.5
210
28.5
240
28.5
270
28.3
300
28.1
Part B #2
Trial (s)
Temp
0
21
30
30.8
60
30.5
90
30.1
120
30
150
30
180
29.9
210
29.8
240
29.5
270
29.1
300
29
Graphs of Temperature vs. Time of Reaction
T
i
from Trial #1: 21
T
f
from Trial #1: 29.64
T
i
from Trial #2: 21
T
f
from Trial #2: 30.86
Part C: Determination of ΔH for the reaction: Mg
(s)
+ HCl
(aq)
MgCl
2(aq) + H
2(g)
.
Mass of Mg(s) used in Trial #1 (in grams): 0.008g
Mass of Mg(s) used in Trial #2 (in grams): 0.008g
Data for Experiment:
Part C #1
Trial (s)
Temp 0
23.9
30
29.2
60
30
90
29.5
120
29.4
150
29.2
180
29.1
210
29
240
29
270
28.9
300
28.9
Part C #2
Trial (s)
Temp
0
21.8
30
24.8
60
25.9
90
27
120
27
150
27.1
180
27.5
210
27.5
240
27.5
270
27.5
300
27.4
Graphs of Temperature vs. Time of Reaction
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T
i
from Trial #1: 23.9
T
f
from Trial #1: 29.9
T
i
from Trial #2: 21.8
T
f
from Trial #2: 27.6
Part E: Determination of ΔH for the reaction: HCl
(aq)
+ NaOH
(aq)
NaCl
(aq)
+ H
2
O
(l)
.
Data for Experiment:
Run 1
Time (s)
Temp
0
24
30
24
60
24.3
90
24.5
120
24.1
150
24.1
180
24.1
210
24
240
24
270
24
300
24
Run 2
Time (s)
Temp
0
22
30
26.5
60
26.3
90
26.1
120
26
150
26
180
26
210
25.9
240
25.9
270
25.9
300
25.9
Run 3
Time (s)
Temp
0
23
30
26.1
60
26.2
90
26.2
120
26.1
150
26
180
26
210
26
240
26
270
26
300
26
Run 4
Time (s)
Temp
0
23
30
249
60
25
90
25
120
25
150
25
180
25
210
24.9
240
24.9
270
24.9
300
24.9
Run 5
Time (s)
Temp
0
23
30
23.2
60
23.2
90
23.2
120
23.1
150
23.1
180
23.1
210
23.1
240
23.1
270
23.1
300
23
Graphs of Temperature vs. Time of Reaction
T
i
from Run #1: 24.44
T
f
from Run #1: 24
T
i
from Run #2: 22
T
f
from Run #2: 26.367
T
i
from Run #3: 23
T
f
from Run #3: 26.216
T
i
from Run #4: 23
T
f
from Run #4: 25.056
T
i
from Run #5: 23
T
f
from Run #5: 23.22
Job’s Plot:
Run
Number
Volume of
HCl (mL)
Volume of
NaOH (mL)
Δ
T (from T
f
- T
i
of
graphs)
1
0.50
3.50
0.44
2
1.00
3.00
4.4
3
2.00
2.00
3.2
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4
3.00
1.00
2.1
5
3.50
0.50
0.22
***(Insert the JOB’s PLOT here. Make sure the graph is properly labeled. See lab manual. You should graph Δ
T (
ᵒ
C) (on the y-axis) vs Volume of HCl (mL) (on the x-axis). You won’t be able to type in the Volume of NaOH (mL) in Excel as a second line for the x-axis. What you can do is insert the graph here. And then type in the line for Volume of NaOH (mL) underneath the graph. Just space it so that the numbers (mL) matches that of the graph.
RESULTS and CALCULATIONS:
Part A: Calibration of Calorimeter.
ΔT (first run) = 7.1
ΔT (second run) = 8
Averaged ΔT = 7.55
1.
Calculated heat loss by the hot water: (Insert value here, include the unit of joules)
2.
Calculated heat gained by the cold water: (Insert value here, include the unit
of joules)
3.
Calculated heat absorbed by the calorimeter: (Insert value here, include the unit of joules)
4.
Heat capacity (C
cal
) of the calorimeter = (Insert value here, include the unit of
J/ºC)
Part C: Determination of ΔH for the reaction: Mg
(s)
+ HCl
(aq)
MgCl
2(aq) + H
2(g)
.
First Run:
ΔT (first run) = (Insert value here, this value comes from your graph above)
1.
Calculated heat gained by the HCl water in the calorimeter (first run): (Insert value here, include the unit of joules)
2.
Calculated heat absorbed by the calorimeter (first run): (Insert value here, include the unit of joules. This value is different than the value for Part A.)
3.
Calculated heat released by the reaction (first run): (Insert value here, include the unit of joules. This value is basically the heat of 1 & 2 added.)
4.
ΔH for the reaction (first run): (Insert value here, include the unit of J/mol. Mg is the limiting reactant.)
Second Run:
ΔT (second run) = (Insert value here, this value comes from your graph above)
1.
Calculated heat gained by the HCl water in the calorimeter (second run): (Insert value here, include the unit of joules)
2.
Calculated heat absorbed by the calorimeter (second run): (Insert value here, include the unit of joules. This value is different than the value for Part
A.)
3.
Calculated heat released by the reaction (second run): (Insert value here, include the unit of joules. This value is basically the heat of 1 & 2 added.)
4.
ΔH for the reaction (second run): (Insert value here, include the unit of J/mol. Mg is the limiting reactant.)
Averaged ΔH for the reaction = (Insert value here, include the unit of J/mol)
Part E: Determination of ΔH for the reaction: HCl
(aq)
+ NaOH
(aq)
NaCl
(aq)
+ H
2
O
(l)
.
ΔT values for reactions at various amount
ΔT (0.005 moles of HCl + 0.035 moles of NaOH) = (Insert value here, this value comes from your graph above)
ΔT (0.010 moles of HCl + 0.030 moles of NaOH) = (Insert value here, this value comes from your graph above)
ΔT (0.020 moles of HCl + 0.020 moles of NaOH) = (Insert value here, this value comes from your graph above)
ΔT (0.030 moles of HCl + 0.010 moles of NaOH) = (Insert value here, this value comes from your graph above)
ΔT (0.035 moles of HCl + 0.005 moles of NaOH) = (Insert value here, this value comes from your graph above)
From the Job’s Plot:
The moles of NaOH and moles of HCl where ΔT is the highest are: (Insert values here, this value comes from your Job’s Plot graph above)
ΔT at the best stoichiometric ratio of NaOH and HCl = (Insert value here, this value comes from your graph above)
Calculation of ΔH for the reaction using the values from the Job’s Plot:
(SHOW ALL CALCULATION STEPS)
1.
Calculated heat gained by the water in the calorimeter: (Insert value here, include the unit of joules, remember to use the best ΔT values from the Job’s Plot.)
2.
Calculated heat absorbed by the calorimeter: (Insert value here, include the unit of joules. Remember to use the best ΔT values from the Job’s Plot.)
3.
Calculated heat released by the reaction: (Insert value here, include the unit of joules. This value is basically the heat of 1 & 2 added.)
4.
ΔH for the reaction at the best stoichiometric ratio of HCl to NaOH: (Insert value here, include the unit of J/mol. the limiting reactant is determined
from the Job’s Plot.)
DISCUSSION:
In the Discussion Section, you take a broad look at your findings and your experiment as
a whole. You present a detailed discussion of the results or findings (explain your results; both good and bad), their implications, and interpretations. This section may include the following components:
A)
A reference to the purpose of the experiment.
B)
A review of the findings - possibly looking up the C)
Possible interpretation of or speculation about findings ΔH values of the reactions above
using the Internet and then discussing why it is good or bad compared to the obtained results.
D)
Limitations of the experiments such as problems, pitfalls, and weakness of methods, etc…
E)
Suggestion of ways to improve the design and circumvent or resolve the problems.
REFERENCES:
1.
Valentin, J. et al, General Chemistry II (Chemistry 1 B) Experiments. (2020 Version).
Evergreen Valley College, San Jose, CA.
POST-LAB QUESTIONS:
1.
Why is the total volume of HCl and NaOH the same for each run in Part E?
(Insert your answer here.)
2.
Use ΔHº formation values from your text book, calculate the ΔHº neutralization for the following reaction:
H
2
SO
4
(aq) + 2NaOH(aq) → 2H
2
O(l) + Na
2
SO
4
(s)
(Insert your answer here.)
3.
When 630.0 mg of a compound is dissolved in 6.00 mL water inside a calorimeter the
temperature increased from 19.0 ˚C to 23.0 ˚C. If the total number of Joules produced by this reaction was 202 Joules, calculate the heat capacity of this calorimeter. (
Specific heat capacity of water = 4.184 J/g˚C; Density of water = 1.00 g/mL)
(Insert your answer here.)
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- Chem 143 Specific Heat Capacity Lab Report Temperature of hot water bath(trial 3): 100 7 (С5) Tw = -9m Final Temperature(trial 3): 23.5 (C6) Analysis 1.) Look at your temperature data tables for the three trials. For each find the highest temperature that your calorimeter reached. This is the final temperature of both the calorimeter and the metal shot. Write this temperature in the data section on the (A6, B6, C6) line. 2.) Calculate the change in temperature of the water in your calorimeter, ATwater. ATWater= Trfinal-Tinitial= (A6, B6, C6)-(A4, B4, C4) Alo=27.2 Blo = 24.4 cle = 23.5 ATWater (trial 1)= (A7) %3D A4= 24.4 34= 21.4 C4= 20.2 ATWater (trial 2)= (B7) %3D ATWater (trial 3)= (C7) 3.) Calculate the amount of energy that went into warming up the water in your calorimeter. We will call this qwater. Use the following equation. 9Water= mWater°C Water"A Twater Here mwater is what you wrote for (A3, B3, C3), cWater=4.184 g.°C J and ATWater=(A7, B7, C7). qWater (trial 1) = x 4.184…arrow_forward2.5 X Bb Quiz 8- Blackbox X Ya SOLUTION: A per X eploymentid=5735112480241329813180832311&eISBN=9781305862883&id=1774598910&snapshot!... Use the References to access important values if needed for this question. A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. In an experiment, a 0.3163 g sample of azulene (C1₁0Hg) is burned completely in a bomb calorimeter. The calorimeter is surrounded by 1.061x10³ g of water. During the combustion the temperature increases from 23.18 to 25.79 °C. The heat capacity of water is 4.184 J g-¹°C-1. MindTap - Cenga X References The heat capacity of the calorimeter was determined in a previous experiment to be 797.7 J/°C. Molar Heat of Combustion = Submit Answer Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of azulene based on these data. C10Hg(s) + 1202(9) 4 H₂O(1) + 10 CO₂(g) + Energy ab Calorimeter…arrow_forward⠀ M Apple Google Disney ESPN Yahoo! Biomedical Careers Program Apple iCloud Yahoo Images Bing Google Wikipedia Facebook Twitter LinkedIn The Weather Channel ☆ & & & & & B COWLv2... b b [References] Use the References to access important values if needed for this question. Consider the reaction ANSWER: prod03-cnow-owl.cengagenow.com Submit Answer kJ/mol G [Review Topics] D2L D2L 4HCI(g) + 0₂(g) →2H₂O(g) + 2Cl₂(g) Using the standard thermodynamic data in the tables linked above, calculate AG for this reaction at 298.15K if the pressure of each gas is 13.94 mm Hg. Retry Entire Group 4 more group attempts remaining D2L D2L Yelp TripAdvisor C D2L M G + 88arrow_forward
- Bookmarks Profiles CHE 2B (D) OWLv2 W Window Tab Ignition wires heat sample Water X genow.com/ilrn/takeAssignment/takeCovalentActivity.do?locator-assignment-take Stirrer Submit Answer OWLV2 | Online teachi Thermometer a Molar Heat of Combustion = Help [Review Topics] (References) Use the References to access important values if needed for this question. A bomb calorimeter, or a constant volume calorimeter, is a device often used to determine the heat of combustion of fuels and the energy content of foods. Insulated Sample Burning Steel outside sample bomb dish chamber Combustion (bomb) calorimeter. X Retry Entire Group Periodic Table X ChatGPT The heat capacity of the calorimeter was determined in a previous experiment to be 981.3 J. C-¹ Assuming that no energy is lost to the surroundings, calculate the molar heat of combustion of heptadecanoic acid based on these data. C17H34 O2 (8) + (49/2) O2(g) → 17H₂O(l) +17CO₂ (g)+ Energy kJ/mol 2 more group attempts remaining X In an experiment,…arrow_forwarduse the data in the first photo to solve for the unknowns in the 2nd photoarrow_forwardHi! This is a lab task. I need help on the last table with missing three values. Thank u very much!arrow_forward
- Use the data to answer only Reaction A.arrow_forwardDate: Period: 011: Calculate the AH for the reaction: C2H4 (g) + H2 (g) => C2H6 (g), from the following data: 1. C2H4 (g) + 302 (g) => 2 CO2 (g) + 2 H2O (1) AH-1411 kJ / mole C2 H6 (g) + 7/2 O2 (g) => 2 CO2 (g) + 3 H2O (1) AH - 1560 kJ / mole 3. H2 (g) + ½ O2 (g) => H2O (1) AH - 285.8 kJ / mole 2.arrow_forwardEsc ||| = OTHERMOCHEMISTRY A student runs two experiments with a constant-volume "bomb" calorimeter containing 1200. g of water (see sketch at right). Calculating heat of reaction from bomb calorimetry data First, a 5.000 g tablet of benzoic acid (C6H,CO₂H) is put into the "bomb" and burned completely in an excess of oxygen. (Benzoic acid is known to have a heat of combustion of 26.454 kJ/g.) The temperature of the water is observed to rise from 16.00 °C to 38.96 °C over a time of 9.2 minutes. 2 4. Next, 5.730 g of acetaldehyde (C₂H₂O) are put into the "bomb" and similarly completely burned in an excess of oxygen. This time the temperature of the water rises from 16.00 °C to 42.19 °C. 84°F Sunny Use this information, and any other information you need from the ALEKS Data resource, to answer the questions below about this reaction: FI Explanation Is this reaction exothermic, endothermic, or neither? 4- F₂ Check 2C₂H4O(g) + 50₂(g) 4CO₂(g) + 4H₂O(g) Be sure any of your answers that are…arrow_forward
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