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 & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter10: Gases And Their Properties
Section: Chapter Questions
Problem 105IL: You have a gas, one of the three known phosphorus-fluorine compounds (PF3, PF3, and P2F4). To find...
Related questions
Question
![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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Ff4a6e19e-8ebd-4d32-a804-01b02d606d69%2Fdbdb73f5-053d-44c5-8fbc-c4228521df9d%2Fi395gkf_processed.jpeg&w=3840&q=75)
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.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 5 steps
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
General Chemistry - Standalone book (MindTap Cour…
Chemistry
ISBN:
9781305580343
Author:
Steven D. Gammon, Ebbing, Darrell Ebbing, Steven D., Darrell; Gammon, Darrell Ebbing; Steven D. Gammon, Darrell D.; Gammon, Ebbing; Steven D. Gammon; Darrell
Publisher:
Cengage Learning
Physical Chemistry
Chemistry
ISBN:
9781133958437
Author:
Ball, David W. (david Warren), BAER, Tomas
Publisher:
Wadsworth Cengage Learning,
Chemistry: Principles and Reactions
Chemistry
ISBN:
9781305079373
Author:
William L. Masterton, Cecile N. Hurley
Publisher:
Cengage Learning
Chemistry
Chemistry
ISBN:
9781305957404
Author:
Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:
Cengage Learning