A gas expands against a variable pressure given by `P = (20)/(V)` (where P in atm and V in L). During expansion from volume of 1 litre to 10 litre, the gas undergoes a change in internal energy of 400 J. How much heat is absorbed by the gas during expansion?
An ideal gas expand against a constant external pressure at 2.0 atmosphere from 20 litre to 40 litre and absorb 10kJ of energy from surrounding . What is the change in internal energy of the system ?
An ideal gas undergoes isobaric expansion at pressure P from volume V_1 to V_2 the work done is :
5 mole of an ideal gas expand isothermally and irreversibly from a pressure of 10 atm to 1 atm against a constant external pressure of 1 atm. w_(irr) at 300 K is :
Assertion :- Internal energy of a real gas may change during expansion at const. temperature. Reason :- Internal energy of a real gas ia function of T & P .
During an adiabatic process, the pressure of a gas is found to be proportional to the cube of its absolute temperature. The ratio C_P//C_V for the gas is
A system undergoes a process in which DeltaU = + 300 J while absorbing 400 J of heat energy and undergoing an expansion against 0.5 bar. What is the change in the volume (in L)?
An ideal gas with pressure P, volume V and temperature T is expanded isothermally to a volume 2V and a final pressure P_i , If the same gas is expanded adiabatically to a volume 2V and a final pressure P_alpha find the value of ratio P_alpha/P_i . The ratio of the specific heats for the gas is 1.67.
One mole of an ideal gas undergoes a change of state (2.0) atm, 3.0 L) to (2.0 atm, 7.0 L) with a change in internal energy (DeltaU) = 30 L-atm. The change in enthalpy (DeltaH) of the process in L-atm :
One mole of non - ideal gas undergoes a change of state (1.0 atm, 3.0L, 200 K ) to (4.0 atm, 5.0L,250 K) with a change in internal energy (DeltaU)=40 L-atm . The change in enthalpy of the process in L-atm ,
NARENDRA AWASTHI-THERMODYNAMICS-Level 1 (Q.31 To Q.60)
