Helium gas (?=1.67) is initially at a pressure of 16 atm, a volume of 1L and a t

Question

Helium gas (?=1.67) is initially at a pressure of 16 atm, a volume of 1L and a temerature of 600K. It is expanded isothermally until its volume is 4L and then compressed at a constant pressure until its volume and temperature are such that an adiabatic compression will return the gas to its original state. Sketch this cycle on a PV diagram. (What I don't understand is how can we compress a gas at a constant pressure and adiabatic compression at the same time.)
Helium gas (?=1.67) is initially at a pressure of 16 atm, a volume of 1L and a temerature of 600K. It is expanded isothermally until its volume is 4L and then compressed at a constant pressure until its volume and temperature are such that an adiabatic compression will return the gas to its original state. Sketch this cycle on a PV diagram. (What I don't understand is how can we compress a gas at a constant pressure and adiabatic compression at the same time.)

Explanation / Answer

that an adiabatic expansion would restore the system to the initial state. as the expansion is isothermal initially we have (16atm,1L,T)---->(4atm,4L,T)----->(4atm,v,4T/V) this should be such that PV^d=constant i.e 16*1^1.67=4*(v)^1.67 solve for v

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