# carter tomlenovich

String nick = new String("hyperlisk");

System.out.println(https://hyperlisk.dev);

### Gases

• Fluid that explains to fill the space that contains it.
• Free molecules undergoing breif, elastic collisons.
• Highly compressible,
• Flows from higher to lower pressure,
• Generally act “ideally”.

### Pressure

Pressure is described as Force Exerted / Area of affected region. Also commonly know as Newtons / m^2

$Pressure = \frac{(kg)(s^-2)}{m}$

This unit is called the Pascal (Pa)

• Units
• IUPAC: Standard Pressure = 100,000 Pa = 1 bar
• mmHg: millimeters of mercury in a barometer = 1 Torr
• $1 Atm = 760 Torr = 101325 Pa = 101.325 kPa = 1.01325$

### The Gas Laws

• The properties of gases were elucidated over many tears by several scientists.
• Pressure-Volume: Robert Boyle and Robert Hooke
• Volume-Temperature: J.A.C. Charles
• Pressure-Temperature: Guiaume Amontons
• $PV = nRT$ <– Ideal Gas Law

### Ideal Gas Law

• Law applies STRICKLY to ideal, non-interacting gases.
• Law applies APPROXIMATELY under condictions where gas molecules interact only weakly.
• Most common gases act like “ideal gases” under typical conditions.

• PV = nRT
• n is Number of moles.
• T is temperature in moles.
• P is pressure
• V is Volume
• Boyles Law:
• If n and T are constant:
• $PV = (nRT) = C$
• $P_1V_1 = P_2V_2$
• Charles’s Law:
• Keeping P and n constant:
• $V (nR/P)T = CT$
• $(V_1/T_1) = (V_2/T_2)$
• Keep P and T constant:
• $(V_1/n_1) = (V_2/N_2)$
• $V = (RT/P)n = Cn$

### Using the Ideal Gas Law

Solve for Volume:

• $V = nRT/P$

Solve for pressure:

• $P = nRT / V$

Solve for amount:

• $n = PV/RT$

### Gas Constants

Value Units Pressure Volume
8.31446 m^3 Pa K mol Pa m^3
8.31446x10^-5 m^3 bar K mol bar m^3
8.31446x10^-2 L bar K mol bar L
62.36358 L Torr K mol Torr L
8.205734x10^-2 L atm K mol Atm L