Calculate the work done by the system in an irreversible (sing step) adiabatic expansion of 2 mole of a polyatomic gas `(gamma= 4//3)` from 300K and pressure 10atm to 1 atm: (in KJ) (Give your answer after multiplying with 2.08).
Calculate the Delta H for the isothermal reversible expansion of 1 mole of an ideal gas from initial pressure of 1.0 bar to a final pressure 0.1 bar at a constant temperature at 273K.
1 mole of an ideal gas A ( C_(v,m)=3R ) and 2 mole of an ideal gas B are (C_(v.m)= (3)/(2)R) taken in a constainer and expanded reversible and adiabatically from 1 litre of 4 litre starting from initial temperature of 320K. DeltaE or DeltaU for the process is (in Cal) (Give your answer after divide with 240)
Calculate work done when 1 mole of an ideal gas is expanded reversibly from 20 L to 40 L at a constant temperature of 300 K.
5 mole of an ideal gas expands isothermally and irreversibly from a pressure of 10 atm to 1 atm against a contant external pressure of 1 atm. W_("irr") at 300K is:
The temperature of 5 moles of a gas is decreased by 2K at constant pressure of 1 atm. Indicate the correct statement
At 27^@C , one mole of an ideal gas ocmpressed isothermally and reversibly from a pressure of 2 atm to 1.0 atm, Choose the correct option from the following
The molar heat capacity at constant volume of a system is 12.41J. mol^(-1) . In an adiabatic expansion the temperature of one mole of that gas falls from 298K to 288K. Calculate the work done by the gas.
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
