This ideal gas law treatment isn't quite correct as the volume changes. The amount of air is the same but the volume it occupies is smaller. Work has also been done on the air.Assume you take 6CI of air at room temperature (21C) and normal atmosphere (14psi) and you want to get it to 1000psi. You get:
P1/T1=P2/T2 (The volume of air is constant)
14PSI/21Deg=1000PSI/T2
T2=1500 Degrees.
If you look at it as essentially an isentropic process (reversible and adiabatic(no heat transfer in or out)) which means no change in entropy, and use the equation for entropy of a gas:
entropy eqn.png
Since delta S equals zero (no change in entropy) the equation can be rearranged to:
T = T0e(Rln(P/P0)/Cp)
Where
T=final temp (degrees Kelvin)
T0=initial temp (degrees Kelvin) = 21+273=294
R= the gas constant = 8.314 kJ/kmol degC
P=initial pressure (pascals) = 101,325
P0=final pressure (pascals) = 6,894,747
Cp=specific heat = 29.248 kJ/kmol degC
A quick plug and crank and:
T= 975.7K or 702.7 degrees C
Still pretty hot.
It is also important to use absolute temperatures particularly when taking any ratios and use consistently SI or Imperial units. Hope this helps.