A 118-mL flask is evacuated, and its mass is measured as 97.129 g. When the flask is filled wit

Name: Problem 102, Chapter 11: Introductory Chemistry
Uploaded: 2024-02-09T14:03:49-08:00
Duration: 1 min 57 s
Channel: David Collins
Description: 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?

step 1 To determine if the gas is pure helium, we need to calculate the molar mass. The molar mass is g

Question

A 118-mL flask is evacuated, and its mass is measured as $97.129 \mathrm{~g}$. When the flask is filled with 768 torr of helium gas at $35^{\circ} \mathrm{C}$, it is found to have a mass of $97.171 \mathrm{~g}$. Is the gas pure helium?

   A 118-mL flask is evacuated, and its mass is measured as $97.129 \mathrm{~g}$. When the flask is filled with 768 torr of helium gas at $35^{\circ} \mathrm{C}$, it is found to have a mass of $97.171 \mathrm{~g}$. Is the gas pure helium?

Introductory Chemistry

Nivaldo J. Tro 6th Edition

Chapter 11, Problem 102

Instant Answer

Solved by Expert David Collins

02/09/2024

Step 1

The mass of the helium gas can be found by subtracting the mass of the empty flask from the mass of the flask filled with helium gas. Mass of helium gas = Mass of filled flask - Mass of empty flask Mass of helium gas = 97.171 g - 97.129 g = 0.042 g Show more…

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A 118-mL flask is evacuated, and its mass is measured as $97.129 \mathrm{~g}$. When the flask is filled with 768 torr of helium gas at $35^{\circ} \mathrm{C}$, it is found to have a mass of $97.171 \mathrm{~g}$. Is the gas pure helium?

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Key Concepts

Molar Mass Determination

This concept involves finding the mass of one mole of a substance. By measuring the mass change when a gas is introduced into a container and using the Ideal Gas Law to compute the number of moles present, one can calculate the gas's molar mass, which helps in identifying or confirming its identity.

Gas Purity Assessment

This involves analyzing the calculated molar mass of a gas sample and comparing it with the expected molar mass of a pure gas. If there is a significant discrepancy, it indicates possible contamination or the presence of other gases, making this analysis a crucial step in verifying gas purity.

Ideal Gas Law

This principle relates the pressure, volume, temperature, and number of moles of a gas through the equation PV = nRT. It is foundational in calculating the amount of gas present under specified conditions and is essential for converting measured pressures, volumes, and temperatures into a corresponding quantity of moles.

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