An ideal gas undergoes a reversible expansion process where its pressure is found to be directly proportional to its volume ( 
). Analyze the following statements about this process:
Text Solution
Verified by ExpertsA
We are given 
,
From the ideal gas law, 
.
.
The process is an expansion, so the volume V increases. Since T is proportional to 
, the temperature T must also increase.
The process is an expansion, which means the volume is increasing ( 
0). Since pressure (P) is always positive, the work done (W) must be positive.
As established in the analysis of statement A , the temperature of the gas increases during this expansion 
. Therefore, the internal energy of the gas must increase. An isothermal process is one where the temperature remains constant.
According to the First Law of Thermodynamics,
.
However, we found that the internal energy increases ( 
).
The heat supplied 
is used for both increasing the internal energy and doing work.
Prepare Smarter with CGP Edu
Get practice questions, solutions, and test series in one place.
Write a Review
Share your experience with this question and solution.
Commentary
Send your comment, doubt, correction, or feedback to admin.
Similar Questions
Explore conceptually related problems