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Thermodynamics Equations

M S 7 questions

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Questions in this quiz (7)

  1. 1S= [blank_start]k[blank_end] ln W

    ΔS = [blank_start]qrev[blank_end]/T
    dS= d qrev/[blank_start]T[blank_end]

    For all liquids, [blank_start]ΔvapH[blank_end]/T[blank_start]b[blank_end] = [blank_start]+85[blank_end] [blank_start]J K-1 mol-1[blank_end]

    [blank_start]ΔS[blank_end]= [blank_start]nR[blank_end] [blank_start]ln[blank_end] [blank_start]Vf[blank_end]/[blank_start]Vi[blank_end] = nR ln [blank_start]Pi/Pf[blank_end]

    [blank_start]ΔSm[blank_end] = [blank_start]Cp,m[blank_end] ln [blank_start]Tf[blank_end]/[blank_start]Ti[blank_end]
    1. Ak
    2. Bqrev
    3. CT
    4. DΔvapH
    5. Eb
    6. F+85
    7. GJ K-1 mol-1
    8. HnR
    9. Iln
    10. JVf
    11. KVi
    12. LPi/Pf
    13. MCp,m
    14. NTf
    15. OTi
    16. PΔSm
    17. QΔS
  2. 2For a perfect gas, [blank_start]Cp[blank_end] = [blank_start]Cv[blank_end] + [blank_start]n[blank_end]R

    If monatomic: Cv,m = [blank_start]3/2[blank_end] R Cp,m=[blank_start]5/2[blank_end] R
    If polyatomic: Cv,m [blank_start]>[blank_end] 3/2 R Cp,m>5/2 R

    At temps close to 0, [blank_start]Sm[blank_end] = [blank_start]1/3 Cv[blank_end],m
    1. ACp
    2. BCv
    3. Cn
    4. D3/2
    5. E5/2
    6. F>
    7. G1/3 Cv
    8. HSm
  3. 3ΔSsurr = q[blank_start]surr[blank_end]/T
    qsurr=[blank_start]-q[blank_end]system
    At constant pressure, Δ[blank_start]S[blank_end]surr= [blank_start]-[blank_end]Δ[blank_start]H/T[blank_end]
    1. Asurr
    2. B-q
    3. C-
    4. DH/T
    5. ES
  4. 4ΔrSθ = [blank_start]Σv[blank_end]Smθ ([blank_start]products[blank_end]) [blank_start]-[blank_end] ΣvSmθ ([blank_start]reactants[blank_end])
    ΔStotal = ΔS[blank_start]system[blank_end] + [blank_start]ΔSsurroundings[blank_end]. The process is spontaneous if [blank_start]ΔStotal is positive[blank_end].

    Stθ = [blank_start]Sθ298[blank_end] + C[blank_start]p[blank_end] [blank_start]ln T[blank_end]/[blank_start]298[blank_end]
    1. AΣv
    2. Bproducts
    3. C-
    4. Dreactants
    5. Esystem
    6. FΔSsurroundings
    7. GΔStotal is positive
    8. HSθ298
    9. Ip
    10. J298
    11. Kln T
  5. 5Gibbs energy:
    G= [blank_start]H-TS[blank_end]
    ΔG=ΔH[blank_start]-TΔS[blank_end]. It is to do with the system, for a spontaneous reaction, ΔG must be [blank_start]under 0[blank_end].
    ΔG = the maximum [blank_start]NON EXPANSION work[blank_end] that can be obtained from [blank_start]a process[blank_end] at a constant [blank_start]T[blank_end] and [blank_start]p[blank_end]. It doesn't change the [blank_start]volume[blank_end].
    1. AH-TS
    2. B-TΔS
    3. Cunder 0
    4. DNON EXPANSION work
    5. Ea process
    6. FT
    7. Gp
    8. Hvolume
  6. 6Pressure changes:
    For solids or liquids, ΔG = [blank_start]V[blank_end][blank_start]Δ[blank_end][blank_start]p[blank_end]
    For a gas, [blank_start]ΔG[blank_end]= [blank_start]nRT[blank_end] ln [blank_start]Pi[blank_end]/[blank_start]Pf[blank_end]

    ΔrGθ= Σv[blank_start]G[blank_end]mθ (products) - ΣvGmθ ([blank_start]reactants[blank_end])
    ΔrG changes with temperature: ΔrG= [blank_start]ΔrH[blank_end] - [blank_start]TΔrS[blank_end], if we assume ΔrH and S change very little with temperature.
    1. AV
    2. BΔ
    3. Cp
    4. DnRT
    5. EΔG
    6. FPi
    7. GG
    8. Hreactants
    9. ITΔrS
    10. JΔrH
    11. KPf
  7. 7K= ([blank_start]Pc[blank_end]/Pθ)^[blank_start]c[blank_end] / ([blank_start]Pa/Pθ[blank_end])^a (Pb/Pθ0^b
    SO Δr[blank_start]G[blank_end] = [blank_start]-RT[blank_end] ln K

    [blank_start]lnK[blank_end] = [blank_start]-[blank_end]Δr[blank_start]H[blank_end]θ/[blank_start]R[blank_end] [blank_start](1/T)[blank_end] + [blank_start]ΔrS[blank_end]θ[blank_start]/R[blank_end]
    ΣθΔ
    1. APc
    2. Bc
    3. CPa/Pθ
    4. D-RT
    5. EG
    6. FlnK
    7. G-
    8. HH
    9. IR
    10. J(1/T)
    11. KΔrS
    12. L/R

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Description
Quiz on Thermodynamics Equations, created by M S on 12/04/2016.
Author
M S
Language
English
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