2024-05-28T08:22:36+03:00[Europe/Moscow] en true <p>what are the basic assumptions of kinetic theory as applied to an ideal gas</p>, <p>what conditions are necessary for gas to approach ideal behaviour?</p>, <p>what are limitations of ideality @ very high pressures?</p>, <p>what are limitations of ideality @ very low temperatures?</p>, <p>state general gas equation</p>, <p>state Dalton's Law</p>, <p>state Boyle's Law</p>, <p>state Charle's Law</p>, <p>state Avogadro's Law</p>, <p>compare standard and room temperature &amp; pressure</p>, <p>what defines an ideal gas?</p>, <p>determine molar mass of gas via gas equation</p>, <p>determine density of gas via gas equation</p>, <p>find mole fraction of a gas in gas mixture</p> flashcards
H2 Chemistry 7 - Gaseous state

H2 Chemistry 7 - Gaseous state

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  • what are the basic assumptions of kinetic theory as applied to an ideal gas

    1. gas particles in constant state of random continuous motion

    2. Vgas particles negligible compared to Vcontainer

    3. no IMF b/w gas particles

    4. collisions b/w gas particles perfectly elastic, no loss of energy

    5. average gas particles KE ∝ absolute temp(K)

  • what conditions are necessary for gas to approach ideal behaviour?

    real gases tend towards ideal behaviour @

    high temp, low pressure

    high temp, gas particles high KE >

    sufficient energy to overcome IMF b/w gas particles

    low pressure, Vgas large, gas particles spaced far apart >

    Vgas particles negligible compared to Vcontainer

  • what are limitations of ideality @ very high pressures?

    Vgas small, gas particles closer tgt, Vgas particles significant compared to Vcontainer

  • what are limitations of ideality @ very low temperatures?

    gas particles lower KE, have insufficient energy overcome IMF b/w gas particles, IMF become significant >

    ↑ IMF b/w gas particles, collision b/w particles < elastic >

    Vgas ↓, gas particles close tgt w/ < space b/w them, IMF become significant

  • state general gas equation

    pV = nRT,

    as V = RnT/p

    p = gas pressure(Pa/Nm-2)

    V = Vgas in cubic metre(m3)

    n = ngas(mol)

    R = molar gas constant(8.31JK-1mol-1)

    T = gas temp(K)

  • state Dalton's Law

    in mixture of gases that don't react w/ EO, total pressure exerted by gaseous mixture = sum of partial pressures of each individual gas >

    partial pressure of gas in mixture = pressure gas exerts on wall of container if it alone occupies container

  • state Boyle's Law

    @ constant temp, volume(V) of given mass of gas inversely ∝ to its pressure(p)

    V ∝ 1/p; V = k/p

  • state Charle's Law

    @ constant pressure, volume(V) of fixed mass of gas directly ∝ to absolute temp(T) in Kelvin

    V ∝ T; V = kT

  • state Avogadro's Law

    @ constant pressure & temp, volume(V) of gas directly ∝ to no. of moles of gas(n)

    V ∝ n; V = kn

  • compare standard and room temperature & pressure

    s.t.p. 0oC/273K, 1 bar/105 Pa

    molar volume = 22.7dm3

    r.t.p. 20oC/293K, 1 atm/101325 Pa

    molar volume = 24dm3

  • what defines an ideal gas?

    obeys pV=nRT under all conditions of temp & pressure

    obeys all assumptions of kinetic theory of gases

  • determine molar mass of gas via gas equation

    pV = nRT ---(1)

    n = mass / molar mass = m/M ---(2)

    sub (2) in (1), get

    M = mRT/pV

  • determine density of gas via gas equation

    density, x = mass(g)/volume(m3)

    x = m/V, so m = xV --- (1)

    sub (1) in M = mRT/pV, get

    M = x(RT/p), then

    x(gdm-3) = pM/RT

  • find mole fraction of a gas in gas mixture

    given gas A,

    pAV = nART --- (1)

    ptotalV = ntotalRT --- (2)

    (1)/(2), pA / ptotal = nA / ntotal

    so nA / ntotal = mole fraction of gas A in mixture