3) Show your calculations clearly. Suppose you are provided with a 36.55 g sample of potassium chlorate. a. What mass of oxygen should theoretically be released upon heating? b. What mass of potassium chloride residue should theoretically be left over after heating?
3) Show your calculations clearly. Suppose you are provided with a 36.55 g sample of potassium chlorate. a. What mass of oxygen should theoretically be released upon heating? b. What mass of potassium chloride residue should theoretically be left over after heating?
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter4: Stoichiometry Of Chemical Reactions
Section: Chapter Questions
Problem 62E: Which of the postulates of Dalton’s atomic theory explains why we can calculate a theoretical yield...
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![• Use your data to determine the experimental mass percent of oxygen in KClO3. Show your work clearly for
each step in the table below.
Mass of original KClO3 sample =
Mass of KCl residue =
Mass of Oxygen released =
Mass Percent of Oxygen in KClO3
Average Mass Percent Oxygen =
Sample 1
[Mass of crucible, lid + KCIO3] -
[Mass of crucible + lid] =
33.745 g - 32.721 g = 1.024 g
[Mass of crucible, lid + residue
after 2nd heating] -
[Mass of crucible + lid] =
33.314 g - 32.721 g = 0.593 g
Mass of original KCIO3 sample -
Mass of KCl residue =
1.024 g - 0.593 g = 0.431 g
42.090 +39.444
2
Mass Percent of Oxygen (experim- Mass Percent of Oxygen (experim-
ental) = Mass of Oxygen released /ental) = Mass of Oxygen released
Mass of Potassium chlorate used x Mass of Potassium chlorate used x
100 = 0.431 g/ 1.024 g x 100 = 100 = 0.383 g/0.971 g x 100 =
42.090 %
39.444%
81.534
Sample 2
[Mass of crucible, lid + KCIO3] -
[Mass of crucible + lid] =
33.692 g - 32.721 g = 0.971 g
2
[Mass of crucible, lid + residue
after 2nd heating] -
[Mass of crucible + lid] =
33.309 g - 32.721 g = 0.588 g
Mass of original KCIO3 sample -
Mass of KCI residue=
0.971 g - 0.588 g = 0.383 g
= 40.767 %](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7e668758-5eb5-4a31-abf3-86b767cd65de%2Fc2584613-176e-43e7-a376-36cce5dceea3%2F766og0e_processed.jpeg&w=3840&q=75)
Transcribed Image Text:• Use your data to determine the experimental mass percent of oxygen in KClO3. Show your work clearly for
each step in the table below.
Mass of original KClO3 sample =
Mass of KCl residue =
Mass of Oxygen released =
Mass Percent of Oxygen in KClO3
Average Mass Percent Oxygen =
Sample 1
[Mass of crucible, lid + KCIO3] -
[Mass of crucible + lid] =
33.745 g - 32.721 g = 1.024 g
[Mass of crucible, lid + residue
after 2nd heating] -
[Mass of crucible + lid] =
33.314 g - 32.721 g = 0.593 g
Mass of original KCIO3 sample -
Mass of KCl residue =
1.024 g - 0.593 g = 0.431 g
42.090 +39.444
2
Mass Percent of Oxygen (experim- Mass Percent of Oxygen (experim-
ental) = Mass of Oxygen released /ental) = Mass of Oxygen released
Mass of Potassium chlorate used x Mass of Potassium chlorate used x
100 = 0.431 g/ 1.024 g x 100 = 100 = 0.383 g/0.971 g x 100 =
42.090 %
39.444%
81.534
Sample 2
[Mass of crucible, lid + KCIO3] -
[Mass of crucible + lid] =
33.692 g - 32.721 g = 0.971 g
2
[Mass of crucible, lid + residue
after 2nd heating] -
[Mass of crucible + lid] =
33.309 g - 32.721 g = 0.588 g
Mass of original KCIO3 sample -
Mass of KCI residue=
0.971 g - 0.588 g = 0.383 g
= 40.767 %
Transcribed Image Text:3) Show your calculations clearly. Suppose you are provided with a 36.55 g sample of potassium chlorate.
a. What mass of oxygen should theoretically be released upon heating?
b. What mass of potassium chloride residue should theoretically be left over after heating?
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