Could you please solve this question, asap.

Argon gas in the tank monoatomic, was compressed from atmospheric

pressure to $1500$ psig. This was carried out through a three$-$stage compression

process as follows:

a$.$ Adiabatic compression from atmospheric pressure to $500$ psig

b$.$ Isobaric cooling to room temperature $(300K)$

c$.$ Adiabatic compression from $500$ psig to $1000$ psig

d$.$ Isobaric cooling to room temperature $(300K)$

e$.$ Adiabatic compression from $1000$ psig to $1500$ psig

f$.$ Isobaric cooling to room temperature $(300K.$

Calculate:

The number of moles of argon gas in the tank $($use the final state of $1500$ psig,

$7m^3$ and $300K$ for this calculation$)$

Work done and heat transferred in each of the six steps $($Note: Remember, for

an adiabatic process, $P{V}^{}=$ constant, where $=\frac{C_P}{C_V}.)$

Change in internal energy and enthalpy between each intermediate and final

states.