QUESTION 5 In the Dumas method how is the mass of the gas determined? O The mass of the empty bulb/flask is compared with that of the mass of the bulb/flask after heating O The mass is determined mathemathecally using the Ideal gas equation after heating O The mass of the empty bulb/flask is compared with that of the mass of the bulb/flask with the volatile liquid before heating The mass is taken from the number of moles of the gas inside the flask/bulb whe the water is at 100°c

QUESTION 5 In the Dumas method how is the mass of the gas determined? O The mass of the empty bulb/flask is compared with that of the mass of the bulb/flask after heating O The mass is determined mathemathecally using the Ideal gas equation after heating O The mass of the empty bulb/flask is compared with that of the mass of the bulb/flask with the volatile liquid before heating The mass is taken from the number of moles of the gas inside the flask/bulb whe the water is at 100°c

Introductory Chemistry: A Foundation

9th Edition

ISBN:9781337399425

Author:Steven S. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Donald J. DeCoste

Chapter13: Gases

Section: Chapter Questions

Problem 5ALQ

See similar textbooks

Similar questions

Consider these four gas samples, all at the same temperature. The larger boxes have twice the volume of the smaller boxes. Rank the gas samples with respect to: (a) pressure, (b) density, (c) average kinetic energy, and (d) average molecular speed. (Green spheres are He; violet spheres are Ne.)
Liquid oxygen was first prepared by heating potassium chlorate, KClO3, in a closed vessel to obtain oxygen at high pressure. The oxygen was cooled until it liquefied. 2KClO3(s)2KCl(s)+3O2(g) If 171 g of potassium chlorate reacts in a 2.70-L vessel, which was initially evacuated, what pressure of oxygen will be attained when the temperature is finally cooled to 25C? Use the preceding chemical equation and ignore the volume of solid product.
5.18 When helium escapes from a balloon, the balloon’s volume decreases. Based on your intuition about stretching rubber, explain how this observation is consistent with the gas law.
Nitrogen monoxide gas reacts with oxygen gas to produce nitrogen dioxide gas. What volume of nitrogen dioxide is produced from the reaction of 1 L nitrogen monoxide gas with 3 L oxygen gas? What volume, if any, of the reactants will remain after the reaction ends? Assume all volumes are measured at the same pressure and temperature.
Potassium peroxide is used to absorb the CO2 produced by the people in a space vehicle. 2K2O2(s)+2CO2(g)2K2CO3(s)+O2(g)If a person at rest exhales 3.0 L of air per minute and CO2 is 3.4% (by volume) of exhaled air, how many grams of K2O2 are needed per person for a five-day trip. Assume a temperature of 250 and 728 mm Hg pressure.