CHEM 142 ZOLLER L_1
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Folex Taqll 2009 CHeM 1942 %W 142 20\~ Name: Emily Wiechers Lab Partner: Jeff Sun EXPERIMENT 2: Chemical Composition of Compounds 1. IDENTIFICATION BASED ON PERCENT METAL COMPOSITION 1l. DETERMINATION OF PERCENT KCIO, IN A KCIOy/KCI MIXTURE Grading: This template = 30 pts Lab Notebook pages = 5 pts By signing below, you certify that you have not falsified data and that you have not plagiarized any part of this lab report. Signature: %]/N Purpose and Method Things to think about: What is the.goal of this experiment? Explain how it is accomplished. What is the general methogl (not step by step detailed procedure) that you will be using to achieve this goal? How will you process the data that you record in lab? (What calculations will you use and how do you obtain alt of the values to plug into those equations?) '\ Q\{V\( dwls/ 'QD((K‘\’ in this experiment, Mg is strong heated untit it fully reacts with a component of air (oxygen or nitrogen). Explain how percent Mg is determined. Also explain how percent Mg Is used to distinguish betwoen MgOQ and Mg;N,. (2 pts) In this experiment, percent Mg is determinad by dividing the mass of magnesium by the mass of the product (what is left after burning the Mg) and then multiplying that answer by 100 to get a percentage. The percent Mg is used to distinguish between MgO and Mg3N2 because MgQO and Mg3N2 will have different mass percents of Mg. To distinguish which sample the Mg is from, find the theoretical percent of Mg in each of the compounds by dividing the molar mass of Mg by the molar mass of the campoun and again multiplying it by 100. By doing this, you can compare your perecnt Mg in the experiment with the compounds to diermine which percent it matches. - How is percent Cu determined in the copper carbonate hydroxide compounds? (2 pts) Percent Cu is determined by first finding the mass of the Cu in the sample. To do this, you first have to multiply the mass of the’ product that you obtain by the %Cu in the compound CuQ divided by 100%. Once you have the mass in the sample, you the divide that number by the mass of the reactant in the experiment and muitiply by 100 to get the percent in the copper carbonate hydroxide compounds. How is parcent KCIO, in a KCIO,/KC| mixture determined? (2 pts) Percent KCIO3 in a KCIO3/KCI mixture is determined by the first calculating the moles of oxygen in the mixture. This is done by simply calculating the mass Jost upon heating and converting it into moles because all of the mass lost was oxygen. Convert the moles of oxygen to moles of KCIO3 using the mole to mole ratio. Once you have that answer, convert males of KCIO3 to grams, using the molar mass of the compound. Divide that mass by the mass of the mixture measured at the beginning of the 7/ experiment and multiply by 100 to get the percent. "5 DATA ). Magnesium . . Note: Not reparting all of your data in the tables provided Mass of empty crucible and cover: 19.705|9 may result in the foss of up to Mass of crucible, cover, and Mg: 19.811]g Mass of Mg: 0.108lg Mass of crucible, cover, and product: 19.878|g Mass of product: 0.173|g il. Copper Mass of empty crucible and cover: 18.501|g Mass of crucible, cover, and sample: 18.608|g Mass of sample: 0.105)g Mass of crucible, cover, and product: 18.579|g Mass of product: 0.078)g . KCHKCIO; mixture Mass of crucible and cover : 21.448|g Mass of crucible, cover, and KCI/KCIO3 mixture: 22.458|g Mass of KCI/KEI03 mixture: 1.01fg Mass of crucible, cover, and product: 22.105]|g Mass lost upon heating : 0.353|g
edm: stamd. den: Calculations and Results I. Magnesium Theoretical % Mg in MgO: Calculation here (1 pt) Calculations may be neatly handwritten. melar mars Mfl X100 molay mars 90 1007, >24:3064. y)poy/- = 09.3027. 40.3059 Theoretical % Mg in Mg;N,: Calculation here (1 pt} Calculations may be neatly handwritten. # Mol MY (molar mase 19D x jpoy. meloy™ marc Mgy v, 2(2‘1-30§g !l!fl) 00Y/. ¢ 9 1504294 4 mgsny, P07 T 72T Your measured % Mg in product: Calculation here (2 pt} Calculations may be neatly handwritten. mage of M9 . mass of prodvet X007 0.10¢9 - _ o 07. 6l 27, ‘o.’ifif 0.412F x)007 t/. Measured %Mg values reported by others in your quiz section: 61.97 62.32 61.184 82.89 60.12 61.27 82.275 63.02 51.7 61.2 72.15 7241 Mean | 62.70908 Standard Deviation (s)| 5.383743 Answor 5031, [ Answer 7. \ Answer /. L Show your calculations for the mean and standard deviation or provide the formula you typed into the cell to have Excel perform the calculation. (2 points) o L U 09+ 02 B9 6012 F (127 ¥ 6223563024 C) b2+ 215 *”-"L' 12 \/“"’ FGl A € (427 -0 0329 (62361 2% (€29~ P20+ (427 b012) 2 ¢ ... . [Fepeat (mean mihu( vdlveyfor 4Nl valveg Y
. Copper Theoretical % Cu in Cuy(CO3)(OH), Calculation here (1 pt). Calculations may be neatly handwritten. 07 *Fmole vitmolar mass v xp molar mass CU5COJ(OH),_ 22(635%9 W 22)-10% 9 (v L0g Arswer [578]. Theoretical % Cu in Cuy(CQ3)z(0H),: Calculation here (1 pt). Calculations may be neatly handwritten. X100y. “MOIC v (molar mqr avd melay mASE Cuy(C0y), (oH) X100/ - 65.309 /. Answer [ 55.3]/. = 3(b3.S8499 ov) 599.669 Lvg (£0;),(0H), Measured % Cu in sample: mafs of «mase mass of reactant .0FBg x0-44g - pred (vox Cv 408 Calculation here {2 pt}. Calculations may be peatly handwritten. LU - .G93¢ x)007- =69.34/. y1007. Answer 7. Measured %Cu values reported by others in your sectiq Mean Standard Deviation (s) Show your calculations for the mean and standard deviation or provide the formula you typed into the cell to have Excel perform the calculation. (2 points) $ee Mmaghesivm cales) ~ pleant. mean - add v all valves, dividc by rvin SHOM - (mean ~valve)?, add p. dEN* vy one Jesr tham +he Wity K lvnplen Weal, e per® of valur take squart root, divid € v ber of valves = 0r) 7
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Find the molar mass of the following chemicals:
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31. Calculate the number of moles of the indicated substance present in each of the following samples.
a. 21.4 mg of nitrogen dioxide
b. 1.56 g of copper(II) nitrate
c. 2.47 g of carbon disulfide
d. 5.04 g of aluminum sulfate
e. 2.99 g of lead(II) chloride
f. 62.4 g of calcium carbonate
32. Calculate the number of moles of the indicated substance present in each of the following samples.
a. 47.2 g of aluminum oxide
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A student has three test tubes containing a metal (M) nitrate solution M(NO3)2 (aq)
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and nothing more to the third tube, but forgets to label the tubes. After this, one
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The Jahn-Teller Effect does not apply.
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ammonia complex.
O chloro complex.
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2. Compounds can only be separated into their component elements by
O breaking chemical bonds
O removing impurities
breaking element bonds
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HẸHỘI NH₂
ANH Đ BaCI
CaCl₂
FeCly
NICI₂ HCI H₂0
K₂ CrO₂
KSCN ANH HEO
Give the correct chemical formula for each of the requested chemicals. Enter the subscripts as normal
characters. Ex: BaCl2
Be sure to enter any necessary parentheses. Hint:
1. After addition of what chemical will you expect to see iron precipitate from the solution?
DMG
2. What chemical will be added to precipitate nickel from the solution?
3. What chemical will be added to selectively precipitate barlum from the solution (leaving the calcium
ions in solution)?
4. What color is calcium oxalate?
5. One of the most common mistakes made by students in the lab is not carefully reading the labels on the
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6. During the iron confirmation test, what chemical will be added to dissolve the FeCl
7. What…
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The missing product from this reaction is
-1
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53
122
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A. 52
122
Xe
B. 54
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13. In a certain chemical reaction, 7.29 g of compound A is added to 5.70 g of
compound B. Once the reaction is complete, 3.60 g of compound A and 1.17 g of
compound B remain. What mass of products was produced ?
0
14a. Report this ordinary number in scientific notation: 123000
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1. On the molecular level, what does it mean for a solid sample to be pure?
2. The computed percent recovery was more than 100%. What does this signify, and what should be done about it?
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The mass spectrum below belongs to a compound that contains:
Relative Intensity
100-
8
90
20-
MS2011-04537CM
0-tbn
Chlorine
Bromine
Fluorine
Oxygen
25
50
75
m/z
maltempl
100
125
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Briefly describe the purpose and
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procedures in the analytical process:
a. Sample preparation
b. Replicate measurements
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M Review | Constants | Periodic
Part B
What is the mass percentage of each element in the compound Al2O3?
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* Question Completion Status:
QUESTION 1
During the experiment, the mass of original sample of compound was 2.965 g, and the mass of copper obtained was 1.006 g.
Based on these numbers, calculate the mass of chlorine in the original sample in grams. Include the unit and three decimal places in your answer.
QUESTION 2
6.
If 1.045 g of copper was obtained in the experiment, how many moles (mol) of copper is this?
Include the unit and five decimal places in your answer.
QUESTION 3
During the experiment, a student calculated the mass of chlorine in the compound to be 1.186 g. How many moles (mol) of chlorine are in the
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