Thermodynamics and Gibbs free energy Flashcards

1
Q

Gibbs free energy (G) occurs

A

energy transfer happens as w and heat - wanting to know amount of work the reaction produces

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2
Q

Gibbs free energy equation

A

DG =DH - TDS

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3
Q

+ve entropy

A

difference from lows entropy (s) to higher entropy (l)

relative no. species increase as reaction goes left to right

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4
Q

spontaneous reaction equation for G

A

DG = G(products) - G(reactant) < 0

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5
Q

convenience of G spontaneous reaction

A

only need to calculate quantities for system and not surrounding

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6
Q

law of mass action

A

concentration of R and P at any point in equilibrium reaction are related by reaction quotient (Q)

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7
Q

in equilibrium equation

A

Q = kc

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8
Q

Use of Q to predict direction of reaction

A

Q < kc - left to right

Q > kc - right to left

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9
Q

kc

A

equilibrium constant

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10
Q

kc equation and Q

A

[P]/[R]

must be e.g A / A(0)

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11
Q

interpretation of equilibrium constant kc

A

R > P
R = P
R < P

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12
Q

R > P

A

kc is a small number

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13
Q

R = P

A

kc is some intermediate number

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14
Q

R < P

A

kc is a big number

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15
Q

connection between G and concentration

A

curve - positive curvature

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16
Q

stage one of curve between G and conc

A

-ve gradient

DG - -ve spontaneous

17
Q

stage 2 of curve between G and conc

A

no gradient

equilibrium - DG = 0

18
Q

stage 3 of curve between G and conc

A

+ve gradient

DG - +ve therefore not occurring at A to B but spontaneous at B to A

19
Q

van’t Hoff isotherm

A

relationship of mass action ratio and G

derived yielding - vigourously

20
Q

equation for van’t Hoff isotherm

A

DG = DG* + RTln(Q)

21
Q

at equilibrium of van’t Hoff isotherm

A

DG* = - RTln(kc)

as DG = 0 and Q = kc

22
Q

predicting kc from DG*

A

kc = e(-DG*/RT) - exponential

23
Q

R

A

gas constant 8.13JK-1 mol-1

24
Q

DG*

A

in standard state