If 0.130 mol of N2 gas effuses through a small hole over the course of one hour, calculate the amount of He that would effuse through the same hole over the same period of time. The molar masses of N2 and He are 28.01 and 4.0026 g · mol 1, respectively. Express your answer in mol to three significant figures ? nHe = mol

If 0.130 mol of N2 gas effuses through a small hole over the course of one hour, calculate the amount of He that would effuse through the same hole over the same period of time. The molar masses of N2 and He are 28.01 and 4.0026 g · mol 1, respectively. Express your answer in mol to three significant figures ? nHe = mol

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter5: Gases

Section: Chapter Questions

Problem 60QAP

See similar textbooks

Similar questions

Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?
Given that a sample of air is made up of nitrogen, oxygen, and argon in the mole fractions 0.78 N2, 0.21 O2, and 0.010 Ar, what is the density of air at standard temperature and pressure?
You have an equimolar mixture of the gases SO2 and O2, along with some He, in a container fitted with a piston. The density of this mixture at STP is 1.924 g/L. Assume ideal behavior and constant temperature and pressure. a. What is the mole fraction of He in the original mixture? b. The SO2 and O2 react to completion to form SO3. What is the density of the gas mixture after the reaction is complete?
perform stoichiometric ca1cu1uions for reactions involving gases as reactants or products.
In the anaerobic oxidation of glucose by yeast, CO2 is produced: If 1.56 L of CO2 were produced at 22.0 C and 0.965 atm, what mass of C6H12O6 is consumed by the yeast? Assume the ideal gas law applied.