Gas Laws & Ideal Gas Laws

Molar mass from Ideal Gas Laws

PV= mRT/M or M= mRT/PV M = molar mass of gas m= grams of gas

R = mm Hg

62.4 L(mm Hg)/mol(K)

R = kPa

8.314 L(kPa)/mol(K)

Density from Ideal Gas Laws

D= m/V D = MP/RT

Boyle's Law

Equation: P1V1 = P2V2 If the temperature (and # particles) of a gas is kept constant, the pressure and volume of a gas are inversely related (as one gets larger, the other gets smaller). Pressure and volume units need to be consistent.

Charles Law

Equation: V1/T1 = V2/T2 or V1T2 = V2T1 If the pressure (and # particles) of a gas is kept constant, the temperature and volume of a gas are directly related (if one gets larger, so does the other). Temperature must be in Kelvin, volume units need to be consistent.

Gay-Lussac's Law

Equations: P1/T1 = P2/T2 or P1T2 = P2T1 If the volume (and # particles) of a gas is kept constant, the temperature and pressure of a gas are directly related (if one gets larger, so does the other). Temperature must be in Kelvin, pressure units need to be consistent.

Combined Gas Law

Equations: P1V1/T1 = P2V2/T2 or P1V1T2 = P2V2T1 combines the previous 3 equations to allow you to change more than 1 thing: temperature, pressure, or temperature (# particles is kept constant). Temperature must be in Kelvin, volume and pressure units must be consistent.

Ideal Gas Law

Equations: PV = nRT the relationship among the pressure, volume, temperature, and number of moles of a gas, where P = pressure, V = volume, n = # moles, R = ideal gas constant and T = temperature (in Kelvin) R varies with the unit used to measure pressure.

R = atm

0.0821 L(atm)/mol(K)

Molar Volume of a gas

at STP, 1 mole of any gas will occupy 22.4 L of volume. However, you can use the Ideal Gas Law to determine # moles...