Question

If $3.0 \mathrm{L}$ of oxygen gas at $177^{\circ} \mathrm{C}$ is cooled at constant pressure until the volume becomes $1.50 \mathrm{L}$, then what is the final temperature?

   If $3.0 \mathrm{L}$ of oxygen gas at $177^{\circ} \mathrm{C}$ is cooled at constant pressure until the volume becomes $1.50 \mathrm{L}$, then what is the final temperature?

General Chemistry: Principles and Modern Applications

General Chemistry: Principles and Modern Applications

Ralph H. Petrucci,… 11th Edition

Chapter 6, Problem 11

Instant Answer

Solved by Expert David Collins

06/22/2020

Step 1

0 \mathrm{L}$ to $1.50 \mathrm{L}$ at constant pressure. The initial temperature is $177^{\circ} \mathrm{C}$. We need to find the final temperature. We can use Charles's Law, which states that the volume of a gas is directly proportional to its temperature when the Show more…

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If $3.0 \mathrm{L}$ of oxygen gas at $177^{\circ} \mathrm{C}$ is cooled at constant pressure until the volume becomes $1.50 \mathrm{L}$, then what is the final temperature?

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Key Concepts

Constant Pressure Process

A constant pressure process is one in which the pressure of the gas remains unchanged. Under such conditions, the relationship between the gas's volume and temperature is governed by Charles' Law, allowing predictions of how a change in temperature affects volume when pressure is held fixed.

Absolute Temperature (Kelvin)

Gas law calculations require the use of absolute temperature, measured in Kelvin, because this scale starts at absolute zero where no thermodynamic temperature exists. Converting temperatures from Celsius to Kelvin is necessary to correctly apply relationships such as those in Charles' Law.

Charles' Law

Charles' Law states that for a given amount of gas at constant pressure, the volume is directly proportional to its absolute temperature. This means that if the temperature is decreased, the volume will decrease proportionally, and vice versa, with the relationship mathematically expressed as V/T = constant.

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