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Volume of trapped gas = 88.57 mL - moles of O2 = 0.00359 - Pressure of trapped gas = 756 mmHg - Partial pressure collected O2 =732.2 mm Hg.  - temperature = 298.15 K 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.

Volume of trapped gas = 88.57 mL - moles of O2 = 0.00359 - Pressure of trapped gas = 756 mmHg - Partial pressure collected O2 =732.2 mm Hg.  - temperature = 298.15 K 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
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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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-Volume of trapped gas = 88.57 mL

- moles of O2 = 0.00359
- Pressure of trapped gas = 756 mmHg
- Partial pressure collected O2 =732.2 mm Hg. 

- temperature = 298.15 K
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.

After reacting for several seconds, the heat was removed, and the contents of the testube containing the remaining KC103(s), 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.
Transcribed Image Text:After reacting for several seconds, the heat was removed, and the contents of the testube containing the remaining KC103(s), 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.
Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2(s) catalyst, KCIO3(5) completely decomposes into 02(8) and KCl(s). However, MnO2(s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC1O3(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. O2
Transcribed Image Text:Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2(s) catalyst, KCIO3(5) completely decomposes into 02(8) and KCl(s). However, MnO2(s) itself does not take part in the overall chemical reaction. In an experiment to determine the gas constant, 1.300 g of pure KC1O3(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. O2
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