An ideal diatomic gas contracts in an isobaric process from 1.05 m³ to 0.580 m³ at a constant pressure of 1.30 * 10^5 Pa. If the initial temperature is 455 K, find the work done on the gas, the change in internal energy, the energy transfer Q, and the final temperature. (a) the work done on the gas (in J) J (b) the change in internal energy (in J) J (c) the energy transfer Q (in J) J (d) the final temperature (in K) K
Added by Kimberly P.
Close
Step 1
Therefore, ΔU = Q - W. Show more…
Show all steps
Your feedback will help us improve your experience
Adi S and 88 other Physics 101 Mechanics educators are ready to help you.
Ask a new question
Labs
Want to see this concept in action?
Explore this concept interactively to see how it behaves as you change inputs.
Key Concepts
Recommended Videos
An ideal monatomic gas contracts in an isobaric process from 1.25 $\mathrm{m}^{9}$ to 0.500 $\mathrm{m}^{3}$ at a constant pressure of $1.50 \times 10^{5} \mathrm{Pa} .$ If the initial temperature is 425 $\mathrm{K}$ , find (a) the work done on the gas, (b) the change in internal energy, (c) the energy transfer $Q,$ and $(\mathrm{d})$ the final temperature.
An ideal monatomic gas expands isothermally from 0.500 $\mathrm{m}^{3}$ to 1.25 $\mathrm{m}^{3}$ at a constant temperature of 675 $\mathrm{K}$ . If the initial pressure is $1.00 \times 10^{5} \mathrm{Pa}$ , find (a) the work done on the gas, (b) the thermal energy transfer $Q$ , and (c) the change in the internal energy.
An ideal diatomic gas expands adiabatically from 0.750 $\mathrm{m}^{3}$ to 1.50 $\mathrm{m}^{3}$ . If the initial pressure and temperature are $1.50 \times 10^{5}$ Pa and 325 $\mathrm{K}$ , respectively, find (a) the number of moles in the gas, (b) the final gas pressure, (c) the final gas temperature, and (d) the work done on the gas.
Recommended Textbooks
University Physics with Modern Physics
Physics: Principles with Applications
Fundamentals of Physics
Transcript
Watch the video solution with this free unlock.
EMAIL
PASSWORD