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Biochem Take 2. > Bioenergetics. > Flashcards

Bioenergetics. Flashcards

1
Q

What are bioenergetics?

A

Bioenergetics predicts whether a process will occur or not.

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2
Q

What are kinetics?

A

Kinetics predicts how quickly or how likely a reaction is to occur.

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3
Q

What is the Km of a reaction?

A

The concentration of substrate when an enzyme is at half Vmax.

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4
Q

What is the Vmax of a reaction?

A

The maximum velocity or rate at which an enzyme can work.

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5
Q

The kinetics of a reaction are primarily concerned with what biological reactions?

A

Enzymatic reactions.

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6
Q

What aspects of a reaction are bioenergetics concerned with?

A

The energy needed for a reaction to occur.

Whether a reaction will occur spontaneously

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7
Q

Knowing the bioenergetics allows us to determine what about a biological reaction?

A

Whether it will occur naturally or not.

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8
Q

What is the 1st law of thermodynamics?

A

The energy of the universe is constant.

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9
Q

What is the 2nd law of thermodynamics?

A

The entropy (disorder) of the universe is increasing.

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10
Q

How do the first 2 laws of thermodynamics affect biological reactions?

A

Whether a reaction will occur naturally or not is dependent upon the 1st 2 laws of thermodynamics.

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11
Q

What does the Gibbs free energy equation allow us to calculate?

A

The change in free energy.

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12
Q

What does the change in free energy depend on?

A

The change in enthalpy and the change in entropy.

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13
Q

What is entropy?

A

A measure of disorder.

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14
Q

What is enthalpy?

A

The heat released or absorbed in a reaction.

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15
Q

What is the Gibbs free energy equation?

A

ΔG = ΔH - T ΔS.

Where ΔG = The change in free energy.

ΔH = The change in enthalpy.

T = Temperature.

ΔS = The change in entropy.

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16
Q

What does delta G represent?

A

The change in free energy.

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17
Q

What is the free energy in a reaction?

A

The amount of energy that is available to do work.

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18
Q

As a reaction approaches equilibrium, what will happen to delta G?

A

It will start to approach 0.

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19
Q

What is delta G when a reaction is at equilibrium?

A

0.

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20
Q

What will dictate whether a reaction will occur or not?

A

The amount of free energy that is available.

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21
Q

What is delta G dependent on?

A

The concentrations of products and reactants.

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22
Q

What is delta ΔG°?

A

ΔG° predicts the change in free energy under standard conditions.

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23
Q

How does the addition of ΔG° to the Gibbs free energy equation change the overall equation?

A

ΔG = ΔG° + RT ln (B/A).

Where ΔG = The change in free energy.

ΔG°= The change in free energy under standard conditions.

R = The gas constant.

T = Temperature.

B = Products.

A = Reactants.

24
Q

What are standard conditions for ΔG°?

A

1 mol/litre.

25
Q

What is the other name that ΔG° is known as?

A

The standard free energy change.

26
Q

Can ΔG can be different to the amount of ΔG°?

A

Yes.

27
Q

What does ΔH represent?

A

The change in enthalpy.

28
Q

What does ΔS represent?

A

The change in entropy.

29
Q

Can enthalpy or entropy be used to determine whether a reaction will be spontaneous or not?

A

No.

30
Q

What happens to the reactants in a reaction?

A

They will react to form products.

31
Q

Do reactants contain more energy than products?

A

Yes.

32
Q

What kind of ΔG must a reaction have if it is spontaneous?

A

A negative ΔG.

33
Q

What kind of ΔG must a reaction have if it is not spontaneous?

A

A positive ΔG.

34
Q

Do spontaneous reactions need any energy?

A

No.

35
Q

Are exergonic reactions spontaneous or non spontaneous?

A

They are spontaneous.

36
Q

Do exergonic reactions release energy?

A

Yes.

37
Q

What ΔG will exergonic reactions have?

A

Negative.

38
Q

If a reaction has a positive ΔG, will the products or reactants contain more energy?

A

The products will have more energy.

39
Q

Will a reaction with a positive ΔG be spontaneous or non spontaneous?

A

Non spontaneous.

40
Q

Will a reaction with a positive ΔG be endergonic or exergonic?

A

Endergonic.

41
Q

Does an endergonic reaction require energy before it can take place?

A

Yes.

42
Q

Is there a change in concentration of reactants and products when a reaction is at equilibrium?

A

No.

43
Q

When will a spontaneous reaction stop?

A

When equilibrium has been reached.

44
Q

If the the free energy of A to B is equal to the free energy of B to A, what kind of reaction is it?

A

A reaction at equilibrium.

45
Q

What is a coupled reaction?

A

An overall reaction that is made up of a series of steps of sub reactions.

46
Q

What is a common intermediate?

A

This is an intermediate in a coupled reaction that takes part in all of the steps in a reaction.

47
Q

What is the common intermediate in the following reaction?

Reaction 1. A + B → C + D.
Reaction 2. D + X → Y + Z.

A

D.

48
Q

How do you calculate ΔG for a coupled reaction?

A

You add the delta Gs of both reactions together.

49
Q

If a coupled reaction is made up of a positive ΔG reaction and a negative ΔG reaction will it be spontaneous?

A

Only if the overall reaction has a negative ΔG.

50
Q

Which bonds in ATP have the most energy?

A

The first 2 phosphate bonds.

51
Q

What is ATP made up of?

A

An adenosine which is bound to 3 inorganic phosphates.

52
Q

What is the ΔG of the 1st 2 phosphate groups in ATP?

A

-7300 cal/mol.

53
Q

What is the ΔG of the 3rd phosphate group ATPs in ATP?

A

-4000 cal/mol.

54
Q

What is the ΔG of ATP - ADP?

A

-7300 cal/mol.

55
Q

What is the ΔG of ADP - AMP?

A

-7300 cal/mol.

56
Q

What is the ΔG of AMP - adenosine?

A

-4000 cal/mol.

57
Q

How can we manipulate a reaction to give a -ΔG?

A

By manipulating the concentrations of reactants and products changing a positive ΔG to a negative ΔG?

Biochem Take 2. (24 decks)

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