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Pressure of Gases

 
Pressure is defined a Force per unit area. With gases the force comes from the gas molecules hitting the side of the container. Air pressure is measured with a barometer.

pressure = force / area

P = F / A

Gas pressure is a gauge of the number and force of collisions between gas particles and the walls of the container that holds them. The SI unit for pressure is the pascal (Pa), but other pressure terms include atmospheres (atms), millimeters of mercury (mmHg), and torr. The following is a list of all of the standard pressure in every unit for pressure. 

1 Atm = 760 torr =760 mmHg = 101.325kPa = 101,325 Pa = 14.7lb/in2  = 29.92 inHg

 

"Atmospheric Pressure" is defined as the force per unit area exerted against a surface by the weight of the air above that surface. The Diagram below , the pressure at point "X" increases as the weight of the air above it increases. The same can be said about decreasing pressure.

In the mountains there is less air above you so less pressure. Since gases are compressible, this creates an environment in the mountains that has less air per unit volume. It will be harder to breathe in the mountains because there is actually less O2 per volume compared to at sea level.

 

 

 

Pressure Conversion Examples-Highlight to reveal answers

 

Set up

Answers
99.6 kPa  to atm99.6 kPa X

1 atm

101.3 kPa

= 0.983 atm
    
0.983 atm to mmHg0.983 atm X

760 mmHg

1 atm

= 747 mm Hg
    
747 mm Hg to torr

747 mm Hg X

760 torr

760 mmHg

=747 torr
    
747 torr to kPa

747 torrX

101.3 kPa

760 torr

= 99.6 kPa
    
50.0 kPa  to atm50.0 kPa X

1 atm

101.3 kPa

= 0.494 atm
    
2.60 atm to mmHg2.60 atm X

760 mmHg

1 atm

= 1976 mm Hg
    
315 torr to mmHg

315 mm Hg X

760 mmHg

760 torr

=315 mmHg
    
5.0 atm  to kPa5.0 atm X

101.3 kPa

1 atm

= 505 kPa
    
260 mmHg to atm 260 mmHg X

1 atm

760mmHg

= 0.342 atm
    
21.2 kPa to torr

21.2 kPaX

760 torr

101.3 kPa

= 159 torr
 

 

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