Energetics of Key Metabolic Steps Flashcards

1
Q

Free energy change equation?

A

Concentrations must
be in molar units

RT log = 1.36 log

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2
Q

As the substrate concentration increases relative to the product concentration, the log term will become more ____ and ΔG will become more ____.

A

log more negeative, ΔG more negative

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3
Q

As the substrate concentration increases relative to the product concentration which way does the rxn proceed?

A

greater tendency to proceed from left to right

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4
Q

standard free energy chain equals

A

Kʹ′eq is the ratio of products to substrates at equilibrium

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5
Q

what is the TOTAL standard free energy chain

A

This relationship also holds for calculating ΔGT from ΔG for each step.

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6
Q

When you reverse the direction for writing a reaction, you _____ the sign of the standard free energy change.

A

change

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7
Q

how to to calculate the voltage difference between two half reactions?

A

ΔE°ʹ′ = E°ʹ′ (e- acceptor) - E°ʹ′ (e- donor)

The minus sign accounts for the fact that you are reversing the direction of one of the reactions to make it an oxidation. Don’t change the sign twice.

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8
Q

The standard free energy change, from the voltage difference between two half reactions

A

ΔG°ʹ′ = -nFΔE°ʹ′

n is the number of electrons transferred, F = 23.063 kcal/mol•volt, ΔE°ʹ′

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9
Q

the potential
difference in an oxidation reduction reaction

where reactants and products are not 1 M.

A
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10
Q

as the concentration of substrates increase, ΔE ___

A

increases

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11
Q

The actual free energy change can be calculated from

A

ΔG = -nFΔE

the voltage difference between two half reactions for conditions other than the standard state

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12
Q

ΔG, the actual free energy change which can be measured for a reaction running from left to right under a ____ conditions

A

given set of conditions

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13
Q

ΔG°, the free energy change under some ___ conditions

A

standard

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14
Q

Why is ΔG° useful?

A

Can calculate ΔG under any conditions if ΔG° is known.

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15
Q

To convert kcal/mol to kjoules/mol multiply by

A

4.18 kJ/kcal.

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16
Q

Standard State

∆G = ∆G°, when

A

[subst] and [prod] = 1 M

17
Q

all spontaneous reactions have a

A

negative free energy change

18
Q

biochemests standard state

if water is a product or substrate it is defined as

A

55.5 M = H20

19
Q

biochemests standard state

if H+ is a product or substrate it is defined as

A
20
Q

atp hydrolysis

what is the free energy change equation?

A
21
Q

ΔG = 0, the reaction has no tendency for

A

net reaction in either direction

22
Q

A to C free energy change?

A

ΔG°ʹ′1 + ΔG°ʹ′2 = -1.36 log Kʹ′eq(1) –1.36 log Kʹ′eq(2)

= -1.36 log (Kʹ′eq(1) x Kʹ′eq(2))

23
Q

A to C?

A
24
Q

Cannot use ΔG to predict ΔG at a___

A

catalytic site

the environemnt may be different here

25
Q

ΔG = ΔG°ʹ′ + 1.36 log P/S. If a reaction with a (+)ΔG°ʹ′ is to proceed
as written, the ratio of P/S under physiological conditions must be small enough to

A

result in a negative term which more than offsets the positive ΔG°ʹ′

  • in a coupled pathway with a net negative ΔG, the concentrations of substrates will adjust so that all steps have a negative ΔG.*
26
Q

in a coupled pathway with a net negative ΔG, the concentrations of substrates will adjust so that

A

all steps have a negative ΔG.

since P/S has to be small enough

27
Q

how does malate to OAA be spontaneous with a standard free energy thats positive

A

get a P/S small enough to make the actual free energy change to be negative

28
Q

redox

electron transfer often occurs via the transfer of

A

hydrogen atoms

29
Q

redox half reaction

A

The affinity of A for an e- can be measured as the pressure on an e- to flow to A or from AH2 compared to a standard half-reaction.

30
Q

For a redox reaction, the solvent does not normally supply electrons so

A

two half- reactions must be combined, one as a reduction reaction and one as an oxidation.

31
Q

half reactions are always written in the direction of

A

REDUCTION

32
Q

The affinity of an e- acceptor for an electron is measured relative to a reference:

A

The standard hydrogen cell.

33
Q

if e-‘s tend to flow to the right, the E° is

A

positive

34
Q

The more positive the standard reduction potential the greater the___

A

affinity of the e- acceptor for the electron.

35
Q

what does the nernst equation mean

A

he tendency of a redox reaction to go under conditions where the reactants and products are not at 1 M:

36
Q

what is the nernst equation?

A