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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.

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 atm 99.6 kPa X 1 atm 101.3 kPa = 0.983 atm 0.983 atm to mmHg 0.983 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 atm 50.0 kPa X 1 atm 101.3 kPa = 0.494 atm 2.60 atm to mmHg 2.60 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 kPa 5.0 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