The magnitudes of enthalpy changes for irreversible adiabatic expansion of a gas from 1L to 2L is ∆H_(1) and for reversible adiabatic expansion for the same expansion is ∆H_(2) . Then
In a particular experiment, a gas undergoes adiabatic expansion satisfying the equation VT^(3)= constant. The ratio of specific heats is g then the value of 3g is
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).
When 3.0 mole of an ideal diatomic gas is heated and compressed simultaneously from 300K, 1.0 atm to 400K and 5.0atm, the change in entropy is (Use C_(P) = (7)/(2)R for the gas)
A sample of argon of 1 atm pressure and 300K expands reversibly and adiabatically from 1.25 dm^(3) " to " 2.5 dm^(3) . Calculate the approximate enthalpy (in J) change (i) C_(V) for argon is 12.48 JK^(-1) (ii) Assume argon to be an ideal gas (iii) Delta T= 111.5K
2 mole of an ideal mono atomic gas undergoes a reversible process for which PV^(2)=C . The gas is expanded from initial volume of 1L to a final volume of 3L starting from initial temperature of 300K. Find DeltaH for the process
1kg of an ideal gas expands adiabatically from 200 K to 250 K. If the specific heat of the gas at constant volume is 0.8 kJ kg^(-1)K^(-1) , then the work done by the gas is
NARENDRA AWASTHI-THERMODYNAMICS-Level 3 - Match The Column
