ch 8 - The Gas Phase Flashcards
four variables that define the state of a gaseous sample
pressure (P), volume (V), temperature (T), and number of moles (n)
gas pressure units
atmospheres (atm) or millimeters of mercury (mmHg), which are equivalent to torr; SI unit is the pascal (Pa); mathematical relationship between all of these: 1 atm = 760 mmHg = 760 torr = 101.325 kPa
standard temp and pressure (STP)
conditions at 273 K (0 degrees C) and 1 atm; generally used for gas law calculations
standard state conditions
298 K, 1 atm, 1 M concentrations; used when measuring standard enthalpy, entropy, free energy changes and electrochemical cell voltage
ideal gas
represents a hypothetical gas with molecules that have no intermolecular forces and occupy no volume
ideal gas law
PV = nRT; where P = pressure, V = volume, n = number of moles, T = temp, R = ideal gas constant (8.21 x 10^-2 L x atm/mol x K or 8.314 J/K x mol which is derived when SI units of Pa and cubic meters (for volume) are substituted into the ideal gas law
density (fancy p)
ratio of the mass per unit volume of a substance; usually expressed for gases in units of grams per liter; density derived from ideal gas law: PV = nRT; n = m/Molar mass; PV = (m/molar mass) RT and density = m/V = P(molar mass)/RT
how much space does a mole of an ideal gas at STP occupy?
22.4 L
combined gas Law
can be used to relate changes in temp, volume, and pressure of gas: Psub1Vsub1/Tsub1 = Psub2Vsub2/Tsub2; where the subscripts 1 and 2 refer to the two states of the gas; this equation assumes number of moles stays constant
change in volume
Vsub2 = Vsub1[Psub1/Psub2][Tsub1/Tsub2]
change in volume used to find density
density = m/Vsub2
molar mass from density
molar mass = (density at STP)(22.4 L/mol)
Avogadro’s principle
states that all gases at a constant temp and pressure occupy volumes that are directly proportional to the number of moles of gas present; equal amounts of all gases at the same temp and pressure will occupy equal volumes: n/V = k or nsub1/Vsub1 = nsub2/Vsub2; k = a constant; nsub1 and nsub2 = number of moles of gas 1 and gas 2; Vsub1 and Vsub2 = volumes of gases 1 and 2
Boyle’s Law
for a given gaseous sample held at constant temp (isothermal), the volume of the gas is inversely proportional to its pressure: PV = k or Psub1Vsub1 = Psub2Vsub2; k = a constant; subscripts 1 and 2 = different sets of pressure and volume condidtions; in terms of gas law, n and T are constant here… As pressure increases volume decreases
Charles’s Law
states that, at constant pressure, volume of a gas is proportional to its absolute temp in kelvins: V/T = k or Vsub1/Tsub1 = Vsub2/Tsub2; k = proportionality constant; subscripts 1 and 2 = two different sets of temp and volume conditions; n and P (with reference to ideal gas law) are held constant… as temp increases, volume increase