A 118-mL flask is evacuated, and its mass is measured as 97.129 g. When the flask is filled with 768 torr of helium gas at 35 °C, it is found to have a mass of 97.171 g. Is the gas pure helium?
Here, we are going to identify if the gas used in the above problem is pure helium.
From ideal gas equation, we have,
pV = nRT ----(1)
Where, p = pressure
V = volume of the gas
n = number of moles of the gas
R = universal gas constant and its value is 0.0821 L atm K-1 mol-1
T = temperature
Textbook: Introductory Chemistry
Author: Nivaldo J Tro
This textbook survival guide was created for the textbook: Introductory Chemistry, edition: 5. Introductory Chemistry was written by and is associated to the ISBN: 9780321910295. Since the solution to 102P from 11 chapter was answered, more than 986 students have viewed the full step-by-step answer. The full step-by-step solution to problem: 102P from chapter: 11 was answered by , our top Chemistry solution expert on 05/06/17, 06:45PM. This full solution covers the following key subjects: helium, mass, flask, gas, evacuated. This expansive textbook survival guide covers 19 chapters, and 2046 solutions. The answer to “A 118-mL flask is evacuated, and its mass is measured as 97.129 g. When the flask is filled with 768 torr of helium gas at 35 °C, it is found to have a mass of 97.171 g. Is the gas pure helium?” is broken down into a number of easy to follow steps, and 42 words.