Question

why gases such as oxygen used at hospitals are compressed. Why must compressed gases be shielded from high tempretures? what must happen to compressed oxygen before it can be inhaled?

Answer 1

Ideal gas equation was used to explain the theory.

In hospitals they need to supply oxygen to patients in need. They require a huge amount of oxygen gas normally, TTO Gases in general like oxygen occupy alotet of volume. So to store alot of oxygen we apply Pressure to compress it so we can store more volume. We know: Pr=nRT Cideal gas equation) For a given amount of gas (2) lara neden Let the no. of moles be in At a given temperature T² PV = nRT = constant R = Uninersal gas PV = constan constant (PT) (V) = constant

@ @ They must be kept away from high temperature because it will cause the gas to expand and the oxygen tank might blast. Science behind this: Again, pv=nRT for a given amount of gas n=const It's in a constant to nolume cylinder. P = (n.) 2 =const. 2 PTETT to (Internal pressure may increase so much that the tank blasts) Before inhaling the compressed oxygen, it's pressure should be regulated according to the patient's need. High pressure oxygen when inhaled can become fatal.