When heated, potassium chlorate (KCI03) has a melting point of 355 °C and it decomposes in the temperature of 480 °C . Potassium chlorate (KC103(s)) then decomposes to KCI(s) and 02(g) in the presence of Mn02(s) catalyst. Mn02(s) does not participate in the overall chemical process, though. To determine the gas constant, the experiment used 100. mg of Mn02(s) and 1.300 g of pure KCIO3(s), then they were combined together in a test tube and heated over a bunsen burner. The resultant 02(g) product was collected in a 100-mL eudiometer after being bubbled in distilled water at exactly 25 °C (or 298.15 K). The experiment was carried out at a 755 torr barometric pressure. At 25 °C, the water vapor has a vapor pressure of 23.8 mmHg. The heat was removed after a few seconds of reaction, and the contents of the test tube containing the remaining KC103(s), Mn02(s) catalyst, and the KCl product were weighed to be 1.285 g.The liquid level in the eudiometer is 1.36 cm below the reservoir's water level. The trapped gas is 88.57 mL, according to the eudiometer's graduation. i.) Calculate the number of moles produced by the 02(g). The molar mass of 02 gas is 31.9988 grams per mole. ii) What is the pressure of the gas trapped inside the eudiometer? Compute in mmHg units
When heated, potassium chlorate (KCI03) has a melting point of 355 °C and it decomposes in the temperature of 480 °C . Potassium chlorate (KC103(s)) then decomposes to KCI(s) and 02(g) in the presence of Mn02(s) catalyst. Mn02(s) does not participate in the overall chemical process, though. To determine the gas constant, the experiment used 100. mg of Mn02(s) and 1.300 g of pure KCIO3(s), then they were combined together in a test tube and heated over a bunsen burner. The resultant 02(g) product was collected in a 100-mL eudiometer after being bubbled in distilled water at exactly 25 °C (or 298.15 K). The experiment was carried out at a 755 torr barometric pressure. At 25 °C, the water vapor has a vapor pressure of 23.8 mmHg. The heat was removed after a few seconds of reaction, and the contents of the test tube containing the remaining KC103(s), Mn02(s) catalyst, and the KCl product were weighed to be 1.285 g.The liquid level in the eudiometer is 1.36 cm below the reservoir's water level. The trapped gas is 88.57 mL, according to the eudiometer's graduation. i.) Calculate the number of moles produced by the 02(g). The molar mass of 02 gas is 31.9988 grams per mole. ii) What is the pressure of the gas trapped inside the eudiometer? Compute in mmHg units
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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Transcribed Image Text:When heated, potassium chlorate (KC103) has a melting point of 355 °C
and it decomposes in the temperature of 480 °C. Potassium chlorate
(KC103(s)) then decomposes to KCl(s) and 02(g) in the presence of
Mn02(s) catalyst. Mn02(s) does not participate in the overall chemical
process, though. To determine the gas constant, the experiment used
100. mg of Mn02(s) and 1.300 g of pure KCI03(s), then they were
combined together in a test tube and heated over a bunsen burner. The
resultant 02(g) product was collected in a 100-mL eudiometer after
being bubbled in distilled water at exactly 25 °C (or 298.15 K). The
experiment was carried out at a 755 torr barometric pressure. At 25 °C,
the water vapor has a vapor pressure of 23.8 mmHg.
The heat was removed after a few seconds of reaction, and the contents
of the test tube containing the remaining KCI03(s), MnO2(s) catalyst,
and the KCl product were weighed to be 1.285 g.The liquid level in the
eudiometer is 1.36 cm below the reservoir's water level. The trapped gas
is 88.57 mL, according to the eudiometer's graduation.
i.) Calculate the number of moles produced by the 02(g). The molar
mass of 02 gas is 31.9988 grams per mole.
ii) What is the pressure of the gas trapped inside the eudiometer?
Compute in mmHg units
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