the presence of MnO2(s) catalyst, KClO3(s) completely decomposes into O2(g) 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 KClO3(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
Potassium chlorate upon heating melts at 355 °C and decomposes at 480 °C. In the presence of MnO2(s) catalyst, KClO3(s) completely decomposes into O2(g) and KCl(s). However, MnO2(s) itself does not take part in the overall
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 O2 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.
Trending now
This is a popular solution!
Step by step
Solved in 3 steps with 3 images
