1) Explain
what is meant by the terms “isothermal expansion” and “adiabatic
expansion”. In each case...

Question

1) Explain
what is meant by the terms “isothermal expansion” and “adiabatic
expansion”. In each case derive an expression for the work done in
expanding an ideal gas. Derive an expression for the change in
temperature which occurs during adiabatic expansion. 2)

Calculate
the work done on a closed system containing 50 g of argon gas when it
expands reversibly from a volume of 5 L to a volume of 10 L at a 
constant temperature of XXXXXXXXXXK. Relative atomic mass of argon =
39.948
3)

5
L of argon gas at 100 kPa and XXXXXXXXXXK expands reversibly and
adiabatically to twice its initial volume. Calculate the final
pressure, the work done and the change in temperature, given that
Cp/CV = 1.67 for argon.

David · Accepted Answer

Question1: Explain what is meant by the terms 
“isothermal expansion” and “adiabatic 
expansion”. In each case derive an expression for 
the work done in expanding an ideal gas. Derive 
an expression for the change in temperature 
which occurs during adiabatic expansion.
Ans: 
Isothermal expansion- In this process expansion of 
ideal gas is carried out in such a manner that the 
temperature remains constant throughout the process.
Adiabatic expansion- In this process expansion of 
ideal gas is carried out in such a manner that no heat 
can flow from the system to the surrounding or vice 
versa, i.e., the system is completely insulated from the 
surrounding. 
Work done in expanding an ideal gas: 
Work done (W) on an ideal gas in a cylinder when it is 
compressed by constant pressure, pex can be derived as 
follows: 
Volume change = l × A = ΔV= Vf − Vi 
Pressure (p) = Force/aea 
∴ Force on the piston = pex. A 
Work (W) = Force × Distance 
W = pex. A.l 
W =  pex .

1) Explain what is meant by the terms “isothermal expansion” and “adiabatic expansion”. In each case derive an expression for the work done in expanding an ideal gas. Derive an expression for the...

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