I 2026-05-16 14:48

Status: #new

Tags: #chemistry #gasses

Gas Pressure and Volume

Defining Pressure

• Pressure is $\frac{\overrightarrow{F}}{A}$ , which can be represented with moles and temperature for forces, and volume for the area in KMT

Common Units of Measurement and Statements

• ATM - define as normal weather at sea level
• kPa - defined as 1000 pascals (formal unit of pressure)
• mmHg/Torr - defined as millimetre of mercury
• STP: $\mathrm{T}=0^{\circ }C,P=1$ atm
• SATP:$\mathrm{T}={25}^{\circ }C,P=100kPA$

Common Unit Conversions

• 101.325 kPA = 1 ATM = 760 mmHg

Gas Laws

Boyles Laws

${\mathrm{P}}_1{V}_1=P_2{V}_2$

Charles and Gay-Lussac's Laws

$\frac{V_1}{T_1}=\frac{V_2}{T_2}$ , given Pressure is constant
The key difference between Charles and Lussac's is Charles requires a flexible container and Gay-Lussac a rigid one.

Combine Gas Law

$\frac{P_1{V}_1}{T_1}=\frac{P_2{V}_2}{T_2}$
This accounts for pressure, volume and temperature all at the same time

References

5.0 States of Matter and Kinetic Molecular Theory