Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO29) catalyst, KCIO3(9) completely decomposes into O2g) and KCI6). However, MnO26) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC1O3() and 100. mg of MnO26) were mixed in a test tube and heated over a bunsen burner. The resulting O22) product was bubbled in distilled water that is at exactly 25 °C (or 298.15 K) and collected in a 100-mL eudiometer. The experiment was done under a barometric pressure of 755 torr. The vapor pressure of water vapor at 25 °C is 23.8 mmHg. O2 KCIO After the reaction was completed, the contents of the test tube containing the MnO2(s) catalyst and the KC16) product was weighed to be 1.285 g. The level of the liquid inside the eudiometer rests 1.36 cm below the water level in the reservoir. The graduation on the eudiometer (not shown here) indicates that the trapped gas is 88.57 mL. a. Using the mass of the test tube contents before and after the reaction, calculate the number of moles of O2(g) [MW = 31.9988 g/mol] gas produced. %3D b. Determine the pressure of the trapped gas inside the eudiometer in mmHg. c. Determine the partial pressure of the collected O2 in mm Hg.
Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO29) catalyst, KCIO3(9) completely decomposes into O2g) and KCI6). However, MnO26) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC1O3() and 100. mg of MnO26) were mixed in a test tube and heated over a bunsen burner. The resulting O22) product was bubbled in distilled water that is at exactly 25 °C (or 298.15 K) and collected in a 100-mL eudiometer. The experiment was done under a barometric pressure of 755 torr. The vapor pressure of water vapor at 25 °C is 23.8 mmHg. O2 KCIO After the reaction was completed, the contents of the test tube containing the MnO2(s) catalyst and the KC16) product was weighed to be 1.285 g. The level of the liquid inside the eudiometer rests 1.36 cm below the water level in the reservoir. The graduation on the eudiometer (not shown here) indicates that the trapped gas is 88.57 mL. a. Using the mass of the test tube contents before and after the reaction, calculate the number of moles of O2(g) [MW = 31.9988 g/mol] gas produced. %3D b. Determine the pressure of the trapped gas inside the eudiometer in mmHg. c. Determine the partial pressure of the collected O2 in mm Hg.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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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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![Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the
presence of MnO2(6) catalyst, KC1O3() completely decomposes into Ozg) and KCl).
However, MnO26) itself does not take part in the overall chemical reaction. In an
experiment to determine the gas constant, 1.300 g of pure KClO3(-) and 100. mg of
MnO26) were mixed in a test tube and heated over a bunsen burner. The resulting O2(g)
product was bubbled in distilled water that is at exactly 25 °C (or 298.15 K) and collected
in a 100-mL eudiometer. The experiment was done under a barometric pressure of 755
torr. The vapor pressure of water vapor at 25 °C is 23.8 mmHg.
O2
After the reaction was completed, the contents of the test tube containing the MnO2s)
catalyst and the KCI6) product was weighed to be 1.285 g. The level of the liquid inside
the eudiometer rests 1.36 cm below the water level in the reservoir. The graduation on the
eudiometer (not shown here) indicates that the trapped gas is 88.57 mL.
a. Using the mass of the test tube contents before and after the reaction, calculate the
number of moles of O2(g) [MW = 31.9988 g/mol] gas produced.
b. Determine the pressure of the trapped gas inside the eudiometer in mmHg.
c. Determine the partial pressure of the collected O2 in mm Hg.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9e8f1e7c-86ce-4314-bd3c-a742736bebc8%2F7faf4d85-302c-4a2b-af84-a1467a888451%2Fafx8hvh_processed.png&w=3840&q=75)
Transcribed Image Text:Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the
presence of MnO2(6) catalyst, KC1O3() completely decomposes into Ozg) and KCl).
However, MnO26) itself does not take part in the overall chemical reaction. In an
experiment to determine the gas constant, 1.300 g of pure KClO3(-) and 100. mg of
MnO26) were mixed in a test tube and heated over a bunsen burner. The resulting O2(g)
product was bubbled in distilled water that is at exactly 25 °C (or 298.15 K) and collected
in a 100-mL eudiometer. The experiment was done under a barometric pressure of 755
torr. The vapor pressure of water vapor at 25 °C is 23.8 mmHg.
O2
After the reaction was completed, the contents of the test tube containing the MnO2s)
catalyst and the KCI6) product was weighed to be 1.285 g. The level of the liquid inside
the eudiometer rests 1.36 cm below the water level in the reservoir. The graduation on the
eudiometer (not shown here) indicates that the trapped gas is 88.57 mL.
a. Using the mass of the test tube contents before and after the reaction, calculate the
number of moles of O2(g) [MW = 31.9988 g/mol] gas produced.
b. Determine the pressure of the trapped gas inside the eudiometer in mmHg.
c. Determine the partial pressure of the collected O2 in mm Hg.
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