A 1.00-mol sample of hydrogen gas is heated at constant pressure from 300 K to 420 K. Calculate the work done (in kJ) on the gas.
Added by David B.
Step 1
However, we are not given the pressure or the change in volume directly. But we do know that the gas is hydrogen, and we know the initial and final temperatures. We can use the ideal gas law to find the change in volume. The ideal gas law is: PV = nRT Where: P Show more…
Show all steps
Your feedback will help us improve your experience
Pranay Shrivastava and 91 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
Calculate the work done w in kJ for the adiabatic expansion of 1.00 mol of an ideal gas at an initial pressure of 2.00 bar from an initial temperature of 450 K to a final temperature of 300 K. Assume that C(P,m) = 5/2R.
Kudakwashe M.
"Find the work done by the gas on its surroundings if four moles of a gas expand isothermally at 300 K. If the final pressure of the gas is 80% of the initial pressure, find the work done by the gas on its surroundings. [R=8.314 J/mol-K]"
Dharmendra M.
When 1310 $\mathrm{J}$ of heat are added to one mole of an ideal monatomic gas, its temperature increases from 272 $\mathrm{K}$ to 276 $\mathrm{K}$ . Find the work done by the gas during this process.
Recommended Textbooks
University Physics with Modern Physics
Physics: Principles with Applications
Fundamentals of Physics
Transcript
18,000,000+
Students on Numerade
Trusted by students at 8,000+ universities
Watch the video solution with this free unlock.
EMAIL
PASSWORD
