Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2) catalyst, KCIO3() completely decomposes into Oz@ 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 KC1O36) and 100. mg of MNO2«) Were mixed in a testube and heated over a bunsen burner. The resulting Oz@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 testube containing the remaining KC1O3(), the MnO2) catalyst, and the KCl» 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 testube contents before and after the reaction, calculate the number of moles of Oxe [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. d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol- 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 MnO2) catalyst, KCIO3() completely decomposes into Oz@ 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 KC1O36) and 100. mg of MNO2«) Were mixed in a testube and heated over a bunsen burner. The resulting Oz@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 testube containing the remaining KC1O3(), the MnO2) catalyst, and the KCl» 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 testube contents before and after the reaction, calculate the number of moles of Oxe [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. d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol- K-!. 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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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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![Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO26)
catalyst, KC1036) completely decomposes into O2e and KCl). 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 KC1O36)
and 100. mg of MNO26) were mixed in a testube and heated over a bunsen burner. The resulting O2 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 testube containing the
remaining KCIO3(), the MnO2) catalyst, and the KCle 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 testube contents before and after the reaction, calculate the number of moles of
Oze [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 mm Hg.
d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol-K!.
e. Using 0.0821 as the true value for the gas constant, calculate the % error of the experiment to the nearest
whole number.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5e27a625-7f8d-4fd3-999c-a96f08d03573%2F99de1940-0981-4e30-baac-f6842820c493%2Fklp9ceh_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 MnO26)
catalyst, KC1036) completely decomposes into O2e and KCl). 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 KC1O36)
and 100. mg of MNO26) were mixed in a testube and heated over a bunsen burner. The resulting O2 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 testube containing the
remaining KCIO3(), the MnO2) catalyst, and the KCle 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 testube contents before and after the reaction, calculate the number of moles of
Oze [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 mm Hg.
d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol-K!.
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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