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36 Terms

1

stavaová rovnice

pV=nRT

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2

R =

8,314

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3

Vm

22,414

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4

izotermický stav

p1V1 = p2V2

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5

izobarický stav

T1/V1 = T2/V2

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6

izochorický stav

p1/T1 = p2/T2

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7

standartní podmínky

T = 273,15 K, p = 101,325 kPa

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8

1 bar =

100 kPa

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9

termodynamika věc

ΔG = ΔH - TΔS

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10

spalna tepla

ΔH = ∑(ΔH reakt) - (ΔH produktu)

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11

slučovací tepla

ΔH = (ΔH produktu) - ∑(ΔH reakt)

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12

ΔG = 0

rovnováha

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13

ΔG < 0

samovolné

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14

ΔG > 0

nesamovolné

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15

ΔH = 0

atermická

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16

ΔH < 0

exotermická

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17

ΔH > 0

endotermická

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18

gibsovka

ΔG° = ΔG(produkt.) - ΔG(reakt.)

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19

součin rozpustnosti vzorec

K = [A]^m[B]^n, where A and B are the ions in the solution.

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20

elektrodový potenciál - elektroda 1. druhu

E = E° - (RT/ZF)lna where E° is the standard electrode potential

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21

elektrodový potenciál - elektroda 2. druhu

E = E° - (RT/ZF)ln([ox]/[red]) where [ox] and [red] are the concentrations of the oxidized and reduced forms.

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22

1. Faradayův zákon

m = A · I · t where m is the mass of substance, A is the electrochemical equivalent, I is the current, and t is the time.

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23
  1. Faradayův zákon

A = M/ZF where M is the molar mass and Z is the number of electrons transferred.

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24

pH silne kyseliny

pH = -log[H+]

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25

pOH silne kyseliny

pOH = -log[OH-]

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26

pH slabe kyseliny

pH = ½ · (- log(Ka) - log c(H))

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27

pOH slabe kyseliny

pOH = 14 - ½ · (- log(Ka) - log c(H))

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28

pH solí slabých kyselin a silných zásad

pH = ½ (14 + (-log(Ka)) + log c(S)

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29

pH sol silných kyselin a slabých zásad

pH = ½ (14 - (-log(Kb)) - log c(S)

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30

pH solí slabých kyselin a slabých zásad

pH = ½ (14 + pKa - pKb)

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31

pH pufru slabé kyseliny a její soli

pH = pKa + log(c(S)/c(A))

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32

pH pufru slabé zásady a její soli

pH = 14 - pKb + log(c(B)/c(S))

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33

α pro bázi

α = [H2B+]/c(HB)

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34

α pro kyselinu

α = [A-]/c(HA)

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35

Ka

Ka = [H3O+][A-]/[HA]

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36

Kb

Kb = [OH-][H3B+]/[HB]

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