Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2s catalyst, KCIO35) completely decomposes into 029) and KClg). However, MnO2s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KCIO35) and 100. mg of MnO2,) were mixed in a test tube and heated over a bunsen burner. The resulting 02) 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. After reacting for several seconds, the heat was removed, and the contents of the test tube containing the remaining KCIO3(s), the MnO2(s) catalyst, and the KCI(s) 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 Ozg) [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 Og in mmHg. d. From these results, calculate an experimental value for the ideal gas constant, Rin L atm mol-1 K-'. e. Using 0.0821 as the true value for the gas constant, calculate the % error of the experiment to the nearest whole number.
Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2s catalyst, KCIO35) completely decomposes into 029) and KClg). However, MnO2s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KCIO35) and 100. mg of MnO2,) were mixed in a test tube and heated over a bunsen burner. The resulting 02) 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. After reacting for several seconds, the heat was removed, and the contents of the test tube containing the remaining KCIO3(s), the MnO2(s) catalyst, and the KCI(s) 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 Ozg) [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 Og in mmHg. d. From these results, calculate an experimental value for the ideal gas constant, Rin L atm mol-1 K-'. e. Using 0.0821 as the true value for the gas constant, calculate the % error of the experiment to the nearest whole number.
Transcribed Image Text:Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence
of MnO2 catalyst, KCIO3 completely decomposes into 02) and KClg. However, MnO2
itself does not take part in the overall chemical reaction. In an experiment to determine the gas
constant, 1.300 g of pure KCIO3 and 100. mg of MnO2e) were mixed in a test tube and heated
over a bunsen burner. The resulting 02g) 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.
After reacting for several seconds, the heat was removed, and the contents of the test tube
containing the remaining KCIO3(s), the MnO2(s) catalyst, and the KCI(s) 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 O2g) [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 O, in mmHg.
d. From these results, calculate an experimental value for the ideal gas constant,
R in L atm mol-" K-1.
e. Using 0.0821 as the true value for the gas constant, calculate the % error of
the experiment to the nearest whole number.
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![Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence
of MnO2 catalyst, KCIO3 completely decomposes into 02) and KClg. However, MnO2
itself does not take part in the overall chemical reaction. In an experiment to determine the gas
constant, 1.300 g of pure KCIO3 and 100. mg of MnO2e) were mixed in a test tube and heated
over a bunsen burner. The resulting 02g) 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.
After reacting for several seconds, the heat was removed, and the contents of the test tube
containing the remaining KCIO3(s), the MnO2(s) catalyst, and the KCI(s) 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 O2g) [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 O, in mmHg.
d. From these results, calculate an experimental value for the ideal gas constant,
R in L atm mol-" K-1.
e. Using 0.0821 as the true value for the gas constant, calculate the % error of
the experiment to the nearest whole number.](https://content.bartleby.com/qna-images/question/63609da7-c7c1-4c5e-93ce-e53893107bc1/62849aed-98d9-4949-93d2-2c1d5f286761/x7biren_processed.png)
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