   Chapter 5, Problem 5.41QP General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343

Solutions

Chapter
Section General Chemistry - Standalone boo...

11th Edition
Steven D. Gammon + 7 others
ISBN: 9781305580343
Textbook Problem

You have a cylinder of argon gas at 19.8 atm pressure at 19°C. The volume of argon in the cylinder is 50.0 L. What would be the volume of this gas if you allowed it to expand to the pressure of the surrounding air (0.974 atm)? Assume the temperature remains constant.

Interpretation Introduction

Interpretation:

The volume of argon gas if it is allowed to expand to the pressure of surrounding air by 0.974 atm but with constant temperature has to be calculated.

Concept Introduction:

Boyle’s Law:

Boyle’s law states that at a constant temperature (T), the volume (V) of gas is inversely proportional to the applied pressure (P).

Vα1P (at constant T)

For a system involving changes in pressure, Boyle’s law can be written as

PfVf=PiVi (at constant T)

Where,

Pi and Pf are initial pressure  and final pressure respectively

Vi and Vf are initial volume and final volume respectively

Explanation

To Calculate: The volume of helium if the pressure got changed to 499 mmHg but with constant temperature

Given data:

The volume of cylinder filled with argon gas at 19C and 19.8 atm pressure is 50.0 L

The temperature remains constant

Calculation of volume:

Boyle’s law gives that,

PfVf=PiVi (at constant T)

Here,

The initial pressure, Pi = 19.8 atm

The final pressure, Pf = 0.974 atm

The initial volume, Vi = 50

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