Hotrod,
PV=nRT, or, P=nRT/V. T1/V1 = T2/V2 => P1=P2
Smaller T and smaller V; Pressure is the same.
The pressure is imposed by the turbo, the volume (or density) is automatically adjusted to accommodate the temperature change.
Suppose we had a magical intercooler with no frictional losses. What you are proposing is that the pressures on either side of the frictionless cooler are different! How can that be? Why wouldn’t they equilibrate?
Dynoroom,
There is a difference between simply asserting a “basic” concept, and explaining it.
''In the interest of accuracy'', according to the book [ chemical principles by P.W. selwood] Interested Observers formula
is asx backwards.
''Charles' Law---If the absolute temperature T of a gas sample is changed to T2 it will be found that the new volume V2 is related to the old volume V1 by the expression ''
V1/T1 = V2/T2 OR V2=V1 X T2/T1
''This is the mathematical expression for Charles Law which may be stated as follows''
''The volume of a fixed mass of gas varies directly as the absolute temperature provided the pressure does not change''
Charles' Law is volume 1 divided by temp 1 = volume 2 divided by temp 2, not the temp divided by the volume.
I really like this book because it shows problems worked out + charts to look at. A little of chart on sample of hydrogen gas
temp T1 Volume V
deg Kelvin K ml or millimeter
218 420
300 578
385 739
450 868
610 1180
By looking at the 300 and 610 temps and their volumes you can see that by cooling from 610 deg to 300 deg the volume
is half as much
Well I might as well type in some other gas laws copied out of this chemistry book
Boyles Law
''If the pressure P1 exerted by, and on, a gas sample is changed to P2, it will be found that the new volume V2 is related to the old volume V1 by the expression''
P1V1 = P2V1
'' This is the mathematical expression for Boyles Law which may, in words, be stated as follows;''
''The volume of a fixed mass of gas varies inversely as the pressure, provided the temperature does not change.''
'' Boyle's Law may be written as this''
V2= V1 X P1/P2
Chart showing effect of pressure on sample of hydrogen gas at 25 degree C
Pressure P Volume V
mm mercury ml
50.0 884
170 250
310 413
498 88.8
760 58.1
1000 44.1
By looking at the 498 and 1000 pressures and volumes you can see how doubling the pressure shrinks the volume in half
Its getting late, going to post before I lose this, wil post formula for temp pressure and volume later
JL222
p.s. glad I never took chemistry as later chapters or really tough