Understanding Thermodynamics: Key Laws and Gas Behavior
School
Sungkyunkwan University**We aren't endorsed by this school
Course
PHYSICS 134
Subject
Chemistry
Date
Dec 11, 2024
Pages
1
Uploaded by KidEelMaster1152
Midterm report (total 50 points): Thermodynamics of Materials 1Oct. 28, 20201. (6 points) Briefly explain Boyle’s law, Charles’law, and Ideal gas law.2. (10 points) Derive the following equation:Rccvp.3. (10 points) The initial state of a quantity of monatomic ideal gas isP= 2 atm,V= 10 liters, andT= 100 °C. Thegas is isothermally compressed to a volume of 5 liters and is then heated at constant pressure to the volume of7 liters. It undergoes a reversible adiabatic expansion to the volumeV. This volume is such that a reversibleisothermal expansion to a pressure of 2 atm returns the system to its initial state. All of the changes of state areconducted reversibly. Calculate the value ofVand the total work done by or on the gas.4. (10 points) One mole of an ideal gas in an initial stateP= 1 atm andT= 300 K undergoes the following reversiblyconducted cycle: 1) An decrease in pressure at constantVto 0.2 atm, 2) an isobaric compression to 30 K, 3) anincrease in pressure at constantVto 1 atm, 4) an isobaric expansion to the initial state. a) (8 points) Calculatethe amount of work done by or on the gas as a result of the cyclic process and b) (2 points) calculate the maximumand minimum temperatures attained by the gas during the cyclic process.5. (14 points) One mole of a monoatomic ideal gas is subjected to the following sequence of steps: 1) Starting at300 K and 10 atm, the gas expands freely into a vacuum to triple its volume. 2) The gas is next heated reversiblyto 400 K at constant volume. 3) The gas is reversibly expanded at constant temperature until its volume is againtripled. 4) The gas is finally reversibly cooled to 300 K at constant pressure. Calculate the values of the changesinSfor each step.Appendix:N0= 6.0232 x 1023mole‐1,R= 8.3144 J/mole∙K = 0.08206 liter∙atm/mole∙K
