Two moles of a perfect gas undergo the following processes: (a) a reversible isobaric expansion from (1.0 atm , 20.0 L) to (1.0 atm, 40.0 L) (b) a reversible isochroic change of state from (1.0 atm , 40.0L) to (0.5 atm , 40.0 L) (c) a reversible isothermal compression from (0.5 atm,40.0 L ) to (1.0atm, 20.0L) Calculate the magnitude of work (W) done in L.atm
Two moles of a perfect gas undergo the following process: (a) A reversible isobaric expansion from ( 1.0 atm, 20.0 litre) to ( 1.0 atm, 40.0 litre). (b) A reversible isochoric change of state from ( 1.0 atm, 40.0 litre) to ( 1.0 atm, 40.0 litre). (b) A reversible isochoric change of state from ( 1.0 atm, 40.0 litre) to ( 0.5 atm, 40.0 litre). (c) A reversible isothermal compression from ( 0.5 atm, 40.0 litre) to ( 1.0 atm, 20.0 litre). (i) Sketch with labels each of the process on the same P-V diagram. (ii) Calculate the total work (W) and the total heat change (q) involved in the above process. (iii) What will be the value of DeltaU, DeltaH and DeltaS for the overall process?
A gas originally at 1.10atm and 298K underwent a reversible adiabatic expansion to 1.00atm and 287K . What is the molar heat capacity of the gas?
1 mole of an ideal gas undergoes an isothermal reversible expansion form 10 atm to 1 atm at 300 K. What will be the work done ?
What is correcto for an ideal gas undergoing reversible adiabatic expansion reagarding temperture?
For an adiabatic expansion of a perfect gas dP//P is equal to :
One mole of an ideal gas is subjected to adiabatic expansion form initail state of (10"atm",300K) to final pressure of 1 atm against constant external pressure. Which of the following option contain correct change in thermodynamic parameters for the above process. (Given: gamma=(4)/(3))
During an adiabatic reversibly expansion of an ideal gas
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
