Introductory Chemistry: A Foundation
9th Edition
ISBN:9781337399425
Author:Steven S. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Donald J. DeCoste
Chapter9: Chemical Quantities
Section: Chapter Questions
Problem 29QAP: When elemental carbon is burned in the open atmosphere, with plenty of oxygen gas present, the...
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Question
Find the percent yield of magnesium oxide in your experiment.
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Lab 5 Workbook (Empirical Formula) - Microsoft Word (Product Activation Failed)
0.1963g-.1223g 0.074g
Trial 1
4 Words: 446
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Review
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E-1E-5 * 21 ¶
3. Using the law of conservation of mass, calculate the mass of oxygen in the product.
Trial 1
Trial 2
0.9g-0.564g-0.336g
Paragraph
4. What is the experimental percent composition of magnesium and oxygen in the product of your
reaction?
0.1223/0.1963*100=62.30% Magnesium
0.074/0.1963*100= 37.69% Oxygen
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5. Calculate the moles of magnesium used in this experiment.
Trial 1
Atomic mass of magnesium is 24.305 so 0.1223g/24.305-0.005 mole
O E
Trial 2
564/.900 *100=62.67% Magnesium
0.0336/900 37.33% Oxygen
Trial 2
0.564/24.305=0.023 mole
WA
FUSCE
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Transcribed Image Text:nsert
ter
Page Layout
Times New Rom 12
Á A
BIU abe x, x' Ab A
References. Mailings
Font
Aa
S
Lab 5 Workbook (Empirical Formula) - Microsoft Word (Product Activation Failed)
0.1963g-.1223g 0.074g
Trial 1
4 Words: 446
O Type here to search
Review
View
E-1E-5 * 21 ¶
3. Using the law of conservation of mass, calculate the mass of oxygen in the product.
Trial 1
Trial 2
0.9g-0.564g-0.336g
Paragraph
4. What is the experimental percent composition of magnesium and oxygen in the product of your
reaction?
0.1223/0.1963*100=62.30% Magnesium
0.074/0.1963*100= 37.69% Oxygen
Amin
te-
Ad AaBb AaBbC AaBbC AaBbC AaBbC
Heading 1
Heading 2
Heading 3
Heading 4
Heading 5
Heading 9
Styles
5. Calculate the moles of magnesium used in this experiment.
Trial 1
Atomic mass of magnesium is 24.305 so 0.1223g/24.305-0.005 mole
O E
Trial 2
564/.900 *100=62.67% Magnesium
0.0336/900 37.33% Oxygen
Trial 2
0.564/24.305=0.023 mole
WA
FUSCE
140
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anter
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A
References. Mailings
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Lab 5 Workbook (Empirical Formula) - Microsoft Word (Product Activation Failed)
Review
4 Words: 446
View
*# *# 21 ¶
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3--
Paragraph
6. Calculate the moles of oxygen atoms used in this experiment.
Trial 1
Atomic mass of O=16g/mol 0.0740/16g=0.0046 mole
Type here to search
Mole of mag/mol of Ox=0.005/0.0046-1.08 mole
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7. Calculate the ratio between the number of moles of magnesium and the number of moles of oxygen in
the product. What is the calculated empirical formula of magnesium oxide?
Trial 1
Trial 2
Trial 2
0.336/16=0.021 mole
0.023/0.021 1.09 mole
8. What is the actual empirical formula of magnesium oxide?
How does this compare to the formula found by your experimentation?
MgO
9. What is the actual percent composition of magnesium oxide? How does this compare to the percent
composition found in your experiment?
Magnesium is 60.19% and Oxygen 39.81%.
It compares fairyl well because the numbers are not far off from eachother in the least.
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140% -](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F4614d4f8-7903-4487-a57c-d3f486f64e89%2F1bf23dee-1e41-415f-b88a-9311945352d5%2Fzjxsl5e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Insert Page Layout
anter
Times New Rom 12 AA Ал IM)
BIU abe x X A aby?
A
References. Mailings
Font
Lab 5 Workbook (Empirical Formula) - Microsoft Word (Product Activation Failed)
Review
4 Words: 446
View
*# *# 21 ¶
E
3--
Paragraph
6. Calculate the moles of oxygen atoms used in this experiment.
Trial 1
Atomic mass of O=16g/mol 0.0740/16g=0.0046 mole
Type here to search
Mole of mag/mol of Ox=0.005/0.0046-1.08 mole
Ad AaBb AaBbc AaBbC AaBbC AaBbC
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Heading 3
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Heading 91
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7. Calculate the ratio between the number of moles of magnesium and the number of moles of oxygen in
the product. What is the calculated empirical formula of magnesium oxide?
Trial 1
Trial 2
Trial 2
0.336/16=0.021 mole
0.023/0.021 1.09 mole
8. What is the actual empirical formula of magnesium oxide?
How does this compare to the formula found by your experimentation?
MgO
9. What is the actual percent composition of magnesium oxide? How does this compare to the percent
composition found in your experiment?
Magnesium is 60.19% and Oxygen 39.81%.
It compares fairyl well because the numbers are not far off from eachother in the least.
4
SE
A
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140% -
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