Chemistry -Measuring Pressure

1 ATM → ATM

1 ATM

1 ATM → mmHg

760 mmHg

1 ATM → Torr

760 Torr

1 ATM → in.Hg

29.9 in. Hg

1 ATM → lb/in²

14.7lb/in²

1 ATM → Pa

101,325kPa

1 ATM →kPa

101.325 kPa

Boyle’s Law

P1V1=P2V2: As pressure increases, volume decreases. Vice Versa. (Remember what happens when you squeeze a balloon) (T, n constant)

Charles Law

V1/T1=V2/T2. As temperature increases, so will volume and vice versa. (Remember in hotter weathers, tires are more prone to pop bc heat and volume increase) (p,n constant)

Gay-Lussac Law

P1/T1=P2/T2: As Temperature increases, so will pressure (v, n constant)

Combined Gas Law

P1V1/T1=P2V2/T2

Avogadro’s law

V1/N1 = V2/N2

Daltons Law of Partial Pressures

P_total=P₁+P₂+…

STP conditions

T= 0c =273K

P= 1 ATM

1 mol gas = 22.4 l (Molar Volume)