Week 2 Postlab report(1) (1)
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Experiment 2 Post-lab report
This report is to be completed and uploaded individually. All answers
submitted for a grade must be in your own words and reflect your understanding of the material.
Name: Directions: You must type out your answers. Proper subscripting, superscripting and capitalization is expected. Answer questions in complete sentences. You may insert pictures of your calculations (written by hand) or type out the calculation using Word’s equation editor feature. Remember to fully explain all of your answers. I do not interpret what you intended to say. You are graded based on the correctness of the answers you write. You must show your work to earn credit for all calculations.
You must upload the document (in .doc, .docx, .rtf, or .pdf) format when completed. All pictures must be legible and oriented properly to earn credit. Do not provide a link to the document, even in a JWU shared folder. You must upload the actual Word document. It is due at 8 a.m. 1 week from today (when our next experiment begins..
1.
For each experiment, type out the data you recorded in lab. Complete the calculations for all rows as required.
Data Table 1: Density of a Penny by Displacement
Line
Pre-1982 Pennies
Post-1982 Pennies
A.
Mass of Pennies (g)
B.
Volume of Water with Pennies (mL)
C.
Initial Volume of Water (mL)
D.
Volume of Pennies
(cm
3
)
Show your set-up and work, not just the
answer.
E.
Density of Pennies
(g/cm
3
)
You must show your work to get credit.
Data Table 2. Density of marbles by displacement
Line
Data using 5 Marbles
Data using 8 marbles
A.
Mass of Marbles (g)
B.
Volume of Water and Marbles (mL)
C.
Initial Volume of Water (mL)
D.
Volume of Marbles
(cm
3
) Show your set-up and work, not just the
answer.
E.
Density of Marbles
(g/cm
3
) You must show your work to get credit.
Data Table 3: Density of Water Using a Volumetric Flask
Line
A.
Mass of Volumetric Flask with Water (g)
B.
Mass of empty Volumetric Flask (g)
C.
Mass of Water (g)
You must show your work to get credit.
D.
Density of Water
(g/cm
3
)
You must show your work to get credit.
Data Table 4. Density of isopropyl alcohol using volumetric pipets
Line
“10 mL”
“25 mL”
A.
Mass of beaker + isopropyl alcohol (g)
B.
Mass of empty beaker (g)
C.
Mass of isopropyl alcohol (g)
You must show your work to get credit.
D.
Density of Isopropyl Alcohol
(g/cm
3
)
You must show your work to get credit.
2.
In the experiment you determined the mass of a stack of twenty pennies, the volume of a stack of twenty
pennies and the density of a stack of twenty pennies. (a) Using the “pre-1982” penny data, what is the average mass, average volume and average density of a single penny? Show your work. (Hint: When you use average mass/average volume, you get average density.)
(b) How does the average density compare to the density calculated in row E of Table 1? Explain why the two densities are related in this way.
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3.
The known density of water is about 1.00 g/mL at 25
°
C. (a) Calculate the percent error associated between your value and the known value. In order to calculate the value, use the equation: percent error
=
|
known value
−
experimental value
known value
|
x
100%
(b) What do you think is the cause of this percent error? Explain
4.
The known density of isopropyl alcohol is about 0.875 g/mL at 25
°
C. (a) Using the equation from the previous problem, calculate the percent error associated between your “10 mL” value and the known value.
(b) Calculate the percent error between your “25 mL” value and the known value.
(c) Which of your two samples produced more accurate results? Why do you think that is? Fully explain your answer. Consider if the error in a measurement is a smaller percentage of the total volume for a larger or smaller amount of alcohol.
5.
There should be a difference in density between the pre-1982 pennies and the post-1982 pennies. In 1982, they changed the composition of pennies due to cost. The two components found in pennies are copper and zinc. Copper has a density of 8.96 g/cm
3
. Zinc has a density of 7.04 g/cm
3
. Based on your calculated densities, do you think there is more copper or zinc in a pre-1982 penny? Which is there more of in a post-1982 penny, copper or zinc? Fully justify your answers.
6.
Is the density value dependent on the number of marbles (within experimental error)? Explain why or why not.
7.
In the movie, "Raiders of the Lost Ark", Indiana Jones takes a gold idol from a cave. The statue is resting on a table which is rigged with a weight sensor. The weight sensor can detect when the weight is removed and will set off a series of unfortunate accidents. To prevent this from happening, Indiana replaces the gold idol with a bag of sand. The volume of the gold idol is approximately 1.65 L. The density of gold is 19.3 g/mL and the density of sand is 1.5 g/mL. (a) Assuming the idol is pure gold, what volume would the bag of sand have to be in order to weigh exactly the same as the idol and not set off the booby-traps? Show your work.
(b) Let’s assume that Indiana is successful in removing the idol and returning it to his laboratory. He decides to determine if it is really pure gold. He weighs the idol and measures the volume by a water displacement method. The results are: mass = 17.4 kg and volume of water displaced = 846 mL. Is the idol made of pure gold? Explain your answer based on the experimental results. Show all necessary calculations to make your determination
8.
Suppose you are measuring the volume of a volatile liquid (
i.e.
one that evaporates easily). If some of the liquid evaporates between the time the liquid is massed and when the volume was measured, will the
reported density of the liquid be too high, too low, or unaffected? Explain your answer.
9.
Pumice is volcanic rock that contains many trapped air bubbles. A 168 gram sample occupied 146.6 mL. (a) What is the density of pumice? Show your work.
(b) Will pumice float on water? Fully explain your answer.
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10. Write a step by step procedure to determine the density of a wood block. (Caution: wood floats in water.)
11. What were the major experimental sources of error? Never give the answer “human error”. Give at least 2 specific errors that were possible in this experiment. Be specific and base the answer on what you actually did.
12. Consider MASS, VOLUME, and DENSITY. a) Which are extensive, and which are intensive properties? b) Which property is the most useful in helping to identify unknowns and why? Explain
13. A group of students determine the density of a sample of liquid ethylene glycol. Each student uses a graduated cylinder to obtain the ethylene glycol volume and a balance to obtain the ethylene glycol mass. Their density values are
shown in the table below. a)
Determine the average density in
this density data set. Show your
work. b) During the second part
of the laboratory activity, the
students decide to determine the
density of ethylene glycol using a
beaker. The results are displayed
in the graph to the right, along
with those obtained using the graduated cylinder. Which glassware yielded the more precise measurements? Explain.
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2- Lab Report
1 Post-Lab
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How could you distinguish solution of sodium chloride (table salt) from a solution of sodium iodide (a poison) using an AgNO3 solution? Show reactions.
Express your answers as balanced chemical equations. Identify all of the phases in your answer. Seperate the two equations by a comma.
> View Available Hint(s)
Submit
Request Answer
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Provide Feedback
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8r
10
13 140 15
16
20
11
12
17
18
19
20
A Moving to another question will save this response.
Quèstion 6
Select the statement that is not supported by the following equation:
q=0=(mwater)(Cwater)(ATwater)+ (mmetal)(Cmetal)( ATmetal)
The total change in heat is the sum of the changes in heat of water and a metal.
Energy is conserved.
Energy is transferred between water and a metal.
Energy is lost during a calorimetry experiment.
A Moving to another question will save this response.
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O CHEMICAL REACTIONS
Identifying the limiting reactant in a drawing of a mixture
The drawing below shows a mixture of molecules:
key
carbon
hydrogen
nitrogen
sulfur
oxygen
chlorine
Suppose the following chemical reaction can take place in this mixture:
CO(g)+2 H,(9) → CH,OH(9)
Of which reactant are there the most initial moles? Enter its chemical formula:
Of which reactant are there the least initial moles? Enter its chemical formula:
Which reactant is the limiting reactant? Enter its chemical formula:
Explanation
Check
FEB
13
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"Use graph paper in lab book to plot moles S2O82- consumed versus time in seconds and fit with a line of best fit.""To determine the slope of your line do not use any of the data points from your data, use 2 points on your straight line.""Units of rate are M/s so you must calculate rate from the slope of your line (mol/s)"
The first picture is the graph, using the seconds and moles from the second picture.
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STANDARD SAMPLE PREPARATIONS FOR ABSORBANCE & CONCENTRATION DATA
Concentration of stock nickel sulfate hexahydrate solution = .400 Molarity
Sample
Volume
Absorbance
Concentration (In Molarity)
a
5 mL
.179
10 mL
.329
15 mL
.588
20 mL
.760
25 mL
.939
Reference Blank = 0
Please show how to find Molarity, please show
steps. Thank you and stay safe.
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Samuel does another experiment, this time with 5% vinegar and 30% vinegar. He sets up two science fair volcanoes (in no particular order), each with the same temperature, mass of baking soda and volume o
vinegar. But one volcano uses 5% vinegar and the other volcano uses 30% vinegar. He measures the volume of gas production for the'first minute of each reaction, and he records the data below.
Volcano # 1
Volume of gas produced (mL.) vs. Time (s) for Volcano #1
Time
Volume of gas
(s)
produced (ml)
60
E 50
10
20
30
25
8 40
38
46
30
20
Volume of gas
produced (ml)
40
50
50
60
52
of
10
53
20
40
60
80
Time (s)
Volcano # 2
Volume of gas
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Based on the data given answer questions. 1,3, and 5 please ??
Question 2 is already answered to solved 1 and 3
1. Based on your three trials, discuss the precision of your data
2. The actual concentration of the unknown is 0.200 M. (Check with instructor to ensure that this value is accurate.) Calculate the percent error based on the average molarity of your three trials.
Answer: Actual Molarity= 0.200M
Mcalculated = 0.1755M
% error = ( [actual - calculated value]/actual ) *100
Putting values;
= ((0.200 - 0.1755)/0.200 )*100
=
12.25%
3. Based on your answer to (2), discuss the accuracy of your data.
5. 80.0 mL of 0.30 M NaOH and 80.0 mL of 0.30 M HCl are mixed together. What is the approximate pH of the solution —acidic, basic, or neutral? Explain.
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If I (the faculty member) come out of the stockroom with the following basket of reactants: (There may be a few I do not use or
need... sort-of like having broccoli in the basket for making bacon and eggs sunny side up..):
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• hydrogen peroxide
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• 2-methyl-2-butene (fresh bottle, still with its seal unbroken,distilled and stored under nitrogen.
• a cylinder of chlorine gas
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OBSERVATION
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→
#
3
Complete the data table using the calculation process you used to complete
the previous question.
Be sure to keep a copy of the completed table to include in the lab report for
this experiment.
$
Trial
1
Trial
2
Trial
3
Trial
4
Trial
5
4
1.00 M Acetic Acid
volume
HC₂H3O2
25.0 mL
25.0 mL
25.0 mL
25.0 mL
25.0 mL
Q Search
f5
%
moles
5
f6
Mole
Ratio
6
HC₂H3O2
: NaHCO3
3:1
2:1
*All values should contain three (3) significant digits.
1:1
1:2
1:3
U
hp
NaHCO3
Molar Mass: 84.007 g/mol
moles
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*
99+
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mass needed
DO
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1. This question is adapted from Harris 19-D.
Carnosine is a dipeptide whose antioxidant properties protect cells from free radicals. Carnosine was
determined by derivatization with naphthalene-2,3-dicarboxyaldehyde and cyanide followed by
fluorescence detection using excitation at 445 nm and emission at 490. Quantification was by standard
addition. To four aliquots of 20-ul cell lysate were added volumes of 100µM carnosine standard to
generate final concentrations of 0, 1.0, 2.5, and 5.0 µM added carnosine. Solutions were diluted to 70µl
before addition of 15µl of 5 mM naphthalene-2,3-dicarboxyaldehyde and 15µl of 10 mM NaCN.
H
H2N.
OH
Carnosine
HN.
Naphthalene-2,3-
dicarboxyaldehyde
Cyanide
OH
Fluorescent product
HN.
Fluorescence intensity
Concentration (uM) of added carnosine
in final 100 µL
0.0
0.465
1.0
0.698
2.5
1.029
5.0
1.651
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