Find the percent yield of magnesium oxide in your experiment.

Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Find the percent yield of magnesium oxide in your experiment.

 

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0.1963g-.1223g 0.074g
Trial 1
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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
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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
140
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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Lab 5 Workbook (Empirical Formula) - Microsoft Word (Product Activation Failed)
Review
4 Words: 446
View
*# *# 21 ¶
E
3--
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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% -
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 Heading 1 Heading 21 Heading 3 Heading 5 Heading 91 Heading 4 Styles 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 Change Styles 140% -
Expert Solution
Step 1

Since there are two different trials, we have to use find the percent yield for each trial separately. 

We use the below formula to find percent yield

Percent yield= Actual yieldTheoretical yield*100

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