Definition

Explanation

Ideal Gas Equation

$$ PV = nRT $$

P = atm (Atmospheric Pressure) V = liter (Volume) n = moles R = constant (0.08206)

$$ R =L \times atm/mol\times K $$

$$ {P_1V_1\over T_1} = {P_2V_2\over T_2} $$

Manometer

Barometer

Unit Conversion

$$ 1atm=760mmHg=760torr=1.01325\times 10^5Pa=101.325kPa=1.01325bar $$

Partial Pressure

Related with number of moles

Ideal Gas

• No attraction between gas molecules = no intermolecular forces
• Have mass, but no volume