AP Chemistry - Gas Laws

14 flashcards · Other · by luckydog789 (harrison holbrook)

  1. Boyle's law

    P1V1=P2V2P_1V_1=P_2V_2P1​V1​=P2​V2​

  2. Charles's law

    V1T1=V2T2\frac{V_1}{T_1}=\frac{V_2}{T_2}T1​V1​​=T2​V2​​

  3. Guy-Lassac's (Guillaume Amontons's) law

    P1T1=P2T2\frac{P_1}{T_1}=\frac{P_2}{T_2}T1​P1​​=T2​P2​​

  4. Combined gas law

    P1V1T1=P2V2T2\frac{P_1V_1}{T_1}=\frac{P_2V_2}{T_2}T1​P1​V1​​=T2​P2​V2​​

  5. Ideal gas law

    PV=nRTPV=nRTPV=nRT

  6. TTT

    Temperature, in ∘K^{\circ}K∘K ( ∘C+273^{\circ}C + 273∘C+273 , really 237.15 but for this class use 273)

  7. RRR

    Gas constant, given on the test

  8. PPP

    Pressure, in atmatmatm , JJJ (a.k.a. kPakPakPa ), or torrtorrtorr (a.k.a mmHgmmHgmmHg )

  9. VVV

    Volume, in LLL

  10. nnn

    The number of moles of the gas

  11. Avogadro's law

    n1V1=n2V2\frac{n_1}{V_1}=\frac{n_2}{V_2}V1​n1​​=V2​n2​​

  12. Dalton's law (of partial pressures)

    PT=Pa+Pb+Pc...P_T=P_a+P_b+P_c...PT​=Pa​+Pb​+Pc​... , where PTP_TPT​ is the total pressure of the gas, PaP_aPa​ and such are the partial pressures of each fraction (the pressure given by just the molecules of a certain pure gas). Can also be represented as nanT=PaPT\frac{n_a}{n_T}=\frac{P_a}{P_T}nT​na​​=PT​Pa​​ , as the amount of gas is proportional to pressure. Importantly, this does not hold true for volume, as each constituent gas has the same volume as the gas they make up.

  13. Root Mean Square (RMS) velocity of a gas (sometimes but very rarely known as Graham's Law)

    μ=3RTMm\mu=\sqrt{\frac{3RT}{M_m}}μ=Mm​3RT​ ​ , where RRR is the gas constant, in this case 8.314 J mol−1K−18.314 \text{ } J \text{ } mol^{-1}K^{-1}8.314 J mol−1K−1 , MmM_mMm​ is the molar mass of the substance, in kg/molkg/molkg/mol , and TTT is temperature, in kelvin

  14. Graham's Law of Effusion

    rate2rate1=Mm1Mm2\frac{\text{rate}_2}{\text{rate}_1}=\sqrt{\frac{M_{m1}}{M_{m2}}}rate1​rate2​​=Mm2​Mm1​​ ​ , which gives the ratio between the rates of effusion of two gases, where gas 1 is the heavier gas, and molar mass is in g/molg/molg/mol . Related is the rate of effusion for one gas, sometimes (don't really use this) gives as 1M\sqrt{\frac{1}{M}}M1​ ​ , where MMM is the molar mass of the gas