For the constant pressure expansion in Example 3.1, assuming that the gas behaves ideally, calculate the initial and final temperatures for the expansion.
For the constant pressure expansion in Example 3.1, assuming that the gas behaves ideally, calculate the initial and final temperatures for the expansion.
Related questions
Question
Transcribed Image Text:3.5 For the constant pressure expansion in Example 3.1, assuming that the gas behaves ideally, calculate the initial and
final temperatures for the expansion.
Transcribed Image Text:Example 3.1
Calculate the work done for the reversible constant pressure expansion of o.05 moles of helium at 2 atmospheres, from an initial
volume of o.5 L to a final volume of 2.0 L.
For the isobaric expansion, the work done is calculated from Equation 3.14. Using SI units,
w =
-pAV = -2.27 x 10°Pa x (0.002 m³ – 0.0005 m³)
= -341 J
The calculation does not depend on the gas behaving ideally. However, calculation of the initial and final temperatures from the
data given above would require the use of the ideal gas law (Problem 3.5) or another equation of state.
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
This is a popular solution!
Trending now
This is a popular solution!
Step by step
Solved in 2 steps
