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Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2(s) catalyst, KC103(5) completely decomposes into O2(g) and KCl(s). However, MnOz(s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC103(s) and 100. mg of MnO2(s) were mixed in a testube 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. After the reaction was completed, the contents of the testube containing the MnO2(s) catalyst and the KCl(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 testube contents before and after the reaction, calculate the number of moles of Oz(8) [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 02 in mm Hg. d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol-1 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.

Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2(s) catalyst, KC103(5) completely decomposes into O2(g) and KCl(s). However, MnOz(s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC103(s) and 100. mg of MnO2(s) were mixed in a testube 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. After the reaction was completed, the contents of the testube containing the MnO2(s) catalyst and the KCl(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 testube contents before and after the reaction, calculate the number of moles of Oz(8) [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 02 in mm Hg. d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol-1 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.

Chemistry
Chemistry
10th Edition
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
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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Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of Mn02(s) catalyst, KC1O3(s) completely decomposes into O2(g) and KCl(s). However, Mn02(s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC103(s) and 100. mg of MnO2(s) were mixed in a testube 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. After the reaction was completed, the contents of the testube containing the MnO2(s) catalyst and the KCl(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 testube 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 02 in mm Hg. d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol-1 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.
Transcribed Image Text:Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of Mn02(s) catalyst, KC1O3(s) completely decomposes into O2(g) and KCl(s). However, Mn02(s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC103(s) and 100. mg of MnO2(s) were mixed in a testube 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. After the reaction was completed, the contents of the testube containing the MnO2(s) catalyst and the KCl(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 testube 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 02 in mm Hg. d. From these results, calculate an experimental value for the ideal gas constant, R in L atm mol-1 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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