Gas Stoichiometry

Titrations

equivalence point is reached when the quantity of known solution is the exact amount needed for stoichiometric reaction with the solution of unknown concentration

ideal gases

ideal gases consists of particles that have;

  1. particles have no volume (small compared to container

  2. particles exert no forces on each other (neither attracted nor repelled)

  3. kinetic energy is unchanged when gases collide with each other or the walls

pressure=force/area

atmospheric pressure is about 14.7 lb/in2 (psi) or 1 atm

1 atm = 760 torr = 760 mmHg

PV=nRT

P = Pressure (atm)

V = Volume (L)

n = number of moles

R = universal gas constant (0.08206 L x atm / mol x K or 8.314 J / mol x K)

T = temperature (K)

d=m/V, density mass Volume

Molar mass = grams of substance divided by moles of substance M=m/n

therefore; M=mRT/PV

PM=dRT

partial pressure

dalton’s law of partial pressures: the total pressure of a mixture of ideal gases is equal to the sum of the partial pressures of the component gasses

each partial pressure is related to the total pressure of the gas mixture via its mole fraction (X) a unit of concentration defined as the number of moles of a component of a mixture divided by the total number of moles of all components

XA=nA/ntotal

*A is for gas A of a mixture and n=number of moles