Gay-Lussac investigated the relationship between the Pressure of a gas and its temperature. At constant Volume, the pressure of a gas sample is directly proportional to the Kelvin Temperature. The relationship is similar to the Volume-Temperature relationship (Charles's Law). The mathematical statement is as follows:
An example of Gay-Lussac application is an autoclave. This is a chamber that sterilizes medical equipment. A short biography is available for Gay-Lussac here.
Suppose we have the following problem:
A gas cylinder containing explosive hydrogen gas has a pressure of 50 atm at a temperature of 300 K. The cylinder can withstand a pressure of 500 atm before it bursts, causing a building-flattening explosion. What is the maximum temperature the cylinder can withstand before bursting?
Let's rewrite this, identifying the variables:
A gas cylinder containing explosive hydrogen gas has a pressure of 50 atm (P1) at a temperature of 300 K (T1). The cylinder can withstand a pressure of 500 atm (P2) before it bursts, causing a building-flattening explosion. What is the maximum temperature the cylinder can withstand before bursting?
Plugging in the known variables into the following mathematical expression
P1 / T1 = P2 / T2
50 atm / 300 K = 500 atm / T2
50 atm ( T2) = (500 atm) (300 K)
T2 = (500 atm) (300 K) / 50 atm = 3000 K
we find the answer to be 3000 K.
Now lets let you try a problem:
Problem: If the pressure of a chamber was 100 atm at 600 K, what will be the temperature of the chamber if the pressure was raised to 600 atm?
Once you have tried the problem, you may check your results by clicking here
R. H. Logan, Instructor of Chemistry, Dallas County Community College
District, North Lake College.
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All contents copyrighted (c) 1996 R.H. Logan, Instructor of Chemistry,DCCCD All Rights reservedRevised: 4/27/99
Original Date of Creation: 11/10/95
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