Lab 1, Post lab Questions, Measurements and Density
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NAME: Danny Abdullah PARTNER’S NAMES:_______________________
LAB SECTION:__________________ _______________________
Measurements, Significant Figures, and using Density to identify unknowns. Using the information you recorded in your lab notebook answer the following questions. Submit this as a typed report. You can’t handwrite it. Part A: The Precision of Volumetric Glassware
Temperature of you measure water 78 degrees Using the website listed in the procedure what is the excepted density of your water? ___0.9998_____
1.
What are the three densities of water from the 50-mL beaker 1.__0.966___ 2.___0.937___ 3. __0.841_____
2.
What is the average density of water from the 50-mL beaker? _____0.915________
3.
What are the three densities of water from the 100-mL graduated cylinder: 1.__0.829___ 2.__0.839____ 3. ___0.897____
4.
What is the average density of water from the 100-mL graduated cylinder? _____0.869________
5.
What are the three densities of water from the 10-mL volumetric pipet 1.__1.0___ 2.___0.903___ 3. ___0.971____
6.
What is the average density of water from the 10-mL volumetric pipet? _____0.985________
7.
What are the three densities of water from the 50-mL Buret
1.__1.0___ 2.___1.019___ 3. __1.006_____
8.
What is the average density of water from the 50-mL Buret
? ____1.008_________
9.
Of the four average densities that you calculate what one is the closest to the excepted density of your water? __0.9998________________
10. Using the average densities calculated in Part A of the lab as justification, list the volumetric glassware used in increasing order of precision. Fully explain your answer, and use percent error to justify your order.
In increasing order of precision, it would be the beaker, then the pipet, then the graduated cylinder, then the buret. The buret has an extremely small percent error of 0.008% while the beaker has a larger percent error of 9.267%. The buret's trials were the most precise while the beaker's trials were not very precise at all.
Part B: The Density of Aluminum and the Thickness of Foil
11. What is the Exact mass of the aluminum pellets in all 5 trials? should be in grams and have at least 3 significant figures. ____20g___ ___25g____ ___23g____ ____20g___ ____24g___ 12. Volume of the aluminum pellets in all 5 trials?_ __9mL_____ ____7mL___ ____10mL___
____8mL___ ___6mL____ 13. Construct and include (copy and paste) your x-y scatter graph of mass vs. volume with trend line and equation and R
2
value shown.
14. Calculated the density of the aluminum pellets?____________ 15. True density of aluminum? ______2.7________
16. Percent error (show calculation)? ______21.62%_________ 17. How many significant figures are in your density and why?
It would technically be 1 significant figure because the smallest value used to calculate density has 1 significant figure.
18. Mass of the aluminum foil? _______0.96%______
19. Volume of the aluminum foil volume?______2.217_______
20. Calculated
thickness of the aluminum foil?_____0.009_______ 21. Percent error (show calculation)? ________21.62%_______ (2.7-2.22)/2.22 x 100 = 21.62
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Related Questions
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A student performed the same experiment as you. The following data was recorded in their
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Mass of
Final buret volume,
Mg, g
Pbarometric, in Hg PH20, torr
T, °C
ml
0.037
37.52
28.62
17.5
20.0
Calculate the student's experimental value of R. Round your answer to four places after the
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1.20
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O STOICHIOMETRY
Using the Avogadro Number
A penny has a mass of 2.50 g and the Moon has a mass of 7.35 x 10“ kg.
22
Use this information to answer the questions below. Be sure your answers have the correct number of significant digits.
What is the mass of 1 mole of pennies?
Round your answer to 3 significant digits.
How many moles of pennies have a mass equal to the mass
of the Moon?
Round your answer to 3 significant digits.
Explanation
Check
© 2021 McGraw-Hill Education. All Riahts Reserved.
To
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A penny has a mass of 2.50 g and the Moon has a mass of 7.35 × 10*“ kg.
Use this information to answer the questions below. Be sure your answers have the correct number of significant digits.
What is the mass of 1 mole of pennies?
Ox10
How many moles of pennies have a mass equal to the mass
of the Moon?
Explanation
Check
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A 0.611 gram sample of copper is carried through the steps of this experiment. At the completion of the last step, 0.427 grams of copper are recovered. What is the percent recovery of the copper metal?
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8. Chemical change is usually irreversible.
9. Color alone is a physical property. But once a substance changes its color, it may
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10. Volume is an intensive property.
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Experiment 3: Determination of the Average Mass of a Penny
Number of pennies: 5
Mass of pennies (weighed together): 13.2
Mass of penny 1: 2.5
Mass of penny 2: 2.5
Mass of penny 3: 2.6
Mass of penny 4: 2.5
Mass of penny 5: 3.1
please help me with this part and show me all step
??????? ???? ?? ? ?????=??? ?? ?ℎ? ?????????? ?????? ?? ?ℎ? ???? ???????/5
1. Total Mass of five pennies (weighed separately):
2. Average mass of a penny (using mass of five pennies weighed together)
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Chemistry
initial mass of benzoic acid 2g
crude mass 1.45g
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Based on the molecule below with each carbon labeled with sequential numbers, answer the following question:
1
H3C
H
2
с
H ₂
C.
4
3
CH3
5
ين
H₂
C
6
H3C 8
7
C
List the "Quaternary" carbon(s) found in the compound above: (please answer like this in sequential number order: #x, #y, etc...)
10
CH3
CH3
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bD
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Initial Water Volume: 12.70 mL
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Density of Solid: ________________
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Part B
Gather all of your pennies dated before 1982. Then follow the steps to complete the table. Include units as
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1. Record the number of pennies dated before 1982.
2. Weigh (as a group) the pennies dated before 1982. Record the total mass. If you're unfamiliar with
using an electronic balance, watch this video before continuing.
3. Calculate and record the average mass of a single penny. If you need help with the calculation, visit
the averaging data section of the math review e.
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number of pennies
combined mass of the pennies (g)
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121 (OL) Lab 3 Den... V
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1
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i
Lynette Maina
Commer
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LE
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Chem 121(OL) Lab 3: Density of Common Materials
Part C Thickness of Aluminum Foil (For help understanding the calculations read the introduction and procedure)
An experiment performed for Part C to measure the length, width and mass of a piece of aluminum foil gave the following
data. You will use this data to solve for the thickness of aluminum foil using the equation from Part C in the introduction.
Length of foil
Width of foil
Mass of foil
13.10 cm
9.50 cm
9.745 g
Use the data in the table to determine the thickness of your aluminum foil (in cm) using the 2.6989 g/mL for the density of
aluminum then convert this value to meters (m) and micrometers (um).
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QUESTION 7
One mole of particles of any substance contains how many particles?
3 × 10-10
particles
3 x 1010
particles
106 particles
6.02 x 10-23 particles
6.02 x 1023 particles
Click Save and Submit to save and submit. Click Save All Answers to save all ans
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[Review Topics]
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Submit Answer
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would there be in 240. g of washers?
washers
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Chapter: 1 Lesson: 2
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