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BIOL 1101 > Lecture 3: Energy and Enzymes > Flashcards

Lecture 3: Energy and Enzymes Flashcards

1
Q

importance of enzymes

A
  • speed up rates of chemical reactions
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2
Q

phosphatas

A
  • an enzyme that catalyzes the reaction of PO3 from protein
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3
Q

what is energy and its types

A

energy: capacity to do work

kinetic: motion
potential: stores energy

other forms: electrical, thermal, mechanical, chemical
- energy has to be converted cant be destroyed

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4
Q

thermodynamics

A

study of energy and transformations

1) energy can be transformed, but not created nor destroyed: total energy in a system must be constant

2) total disorder of a system and surroundings increases: entropy is a measure of disorder
for example: ice is in order, ice lattice structure VS +heat= water when it has disorder

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5
Q

forms of systems

A

CLOSED: exchanges energy but not matter with surroundings

OPEN: exchanges energy and matter (OUR CELLS!)

ISOLATED: exchanges no energy and no matter

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6
Q

what is disorder

A

random motion

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7
Q

what form of energy is most often converted into

A

thermal:
random motion of molecules
increased heat, increases disorder

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8
Q

to go from order to disorder

A

ORDER (no input of energy)
DISORDER (requires energy)

ORDER-DISORDER: spontaneous
DISORDER-ORDERL requires energy

room analogy:
disorder(messy room) takes energy to clean up (order), but it seems to get messy again without much effort

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9
Q

Spontaneous reactions

A
  • chemical or physical reactions which occur without an input of energy from the surroundings
  • change in enthalpy (change in PE) and entropy (measure of disorder) contributes
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10
Q

When do reactions tend to be more spontaneous

A

when products have less PE than reactants
measured based on two criteria:
1) PE: putting in energy
2) DISORDER: H2O is more disordered than ice (change in entropy)

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11
Q

endothermic vs exothermic

A

endo: reactions that absorb energy
- more PE in products, absorb energy
ex. ice melting (energy content of water is greater than ice)
exo: reactions that release energy
- less PE in products, release energy
ex. combustion (release of heat makes it spontaneous)

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12
Q

free energy

A

portion of energy in system available to do work

Change in free energy (Gibbs free energy) will tell you if its spontaneous or not measured using
1) enthalpy (change in PE)
2) entropy (change in order)

negative delta G= spontaneous reaction

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13
Q

Stable vs unstable energy

A

UNSTABLE
- more free energy
- less stable (can be harnessed)
- greater work capacity

STABLE
- less free energy
- more stable
- less work capacity

  • release of free energy can be used for work
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14
Q

Equilibrium

A
  • maximum stability
  • equilibrium point is reached when reactants are converted back to products and converted back to reactants at equal rates
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15
Q

equilibrium in living systems

A
  • living systems are open
  • free energy is negative (spontaneous)
  • organisms reach equilibrium (free energy=0) when they die
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16
Q

thermodynamics and life

A
  • life is highly ordered suggested that it goes against second law (disorder and spontaneous)
  • living things bring in energy and matter to generate order
  • organisms release heat and byproducts to increase disorder too

cells create order but still follow second law of thermodynamics

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17
Q

metabolic pathways and reactions

A
  • exergonic reaction: where G is negative because products contain less free energy than reactants
  • endergonic reaction: where G is positive because products contain more free energy than reactants

EXERGONIC IS NOT EXOTHERMIC
ENDERGONIC IS NOT ENDOTHERMIC

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18
Q

exergonic vs endergonic

A

exergonic: free energy is released, products have less energy so its -G and spontaneous

endergonic: free energy is gained, products have more so +G and its not spontaneous

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19
Q

catabolism vs anabolism

A

catabolism: exergonic, breaking down

anabolism: endergonic, building up

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20
Q

ATP storage and what process will release free energy

A
  • ATP hydrolysis releases free energy that can be used as a source of energy for the cell
  • mostly stored in mitochondria
21
Q

ATP regeneration

A
  • atp used in coupling reactions must be REPLENISHED
  • done by linking atp synthesis to catabolic reactions
  • atp cycle: continue breakdown and re-synthesis of atp
22
Q

what type of reaction is hydrolysis of ATP

A
  • exergonic reaction
  • it can be coupled to make endergonic reactions proceed spontaneously

REQUIRES ENZYMES

23
Q

what can we do with spontaneous internal cellular reactions

A
  • harness that energy to create ATP
24
Q

ATP/ADP cycle

A

exergonic-catabolic
- reactions supply energy for endergonic reaction producing ATP

exergonic reaction
- hydrolyzing ATP
- provides energy for endergonic reactions in cell

25
Q

breaking down atp

A

spontaneous

26
Q

building atp

A

not spontaneous

27
Q

the role of enzymes in biological reactions

A

a) activation energy=kinetic barrier
b) enzymes reduce activation energy to accelerate reactions
c) enzymes combine with reactants and are released unchanged
d) enzymes reduce the activation energy by inducing the transition state

28
Q

relationship between the speed of a reaction and spontaneous reactions

A

unrelated

29
Q

activation energy

A
  • initial input of energy required to start rxn (even for spontaneous rxns)
30
Q

transition state

A
  • molecules that gain necessary activation energy occupy the transition state
31
Q

problem using heat to speed up reactions

A
  • can damage molecules and cells
32
Q

biological catalysts

A

catalyst: chemical agent that speeds up rate of run without being part of the rcn

enzymes=catalysts
- increase rate by lowering activation energy
- don’t supply free energy

33
Q

induced fit

A
  • once a substrate binds to an enzyme, the enzyme will change its 3D shape
  • enzyme is released unchanged
34
Q

Catalytic cycle of enzymes

A
  • enzymes are recycled

1) substrate binds to enzyme forming an enzyme-substrate complex, transition state is reached
TIGHT BINDING, NOT STABLE

between 1 and 2: hydrolytic reaction, -H2O

2) breakage of bond is catalyzed and products are released
3) enzyme can catalyze another reaction

35
Q

cofactors

A
  • inorganic ions/nonproteins necessary to help the enzyme catalyze its rxn

cofactors: metallic ions
coenzymes: organic cofactors (vitamins)

36
Q

enzyme catalysis

A

during catalysis, the substrate and active site form an INTERMEDIATE TRANSITION STATE

1) brings substrate into close proximity
2) expose reactants to changed environments
3) change the shape of substrate

  • charged a.a. can cause the reaction to move faster
37
Q

what conditions and factors affect enzyme activity

A

1) influence of enzyme and substrate concentration

2) enzyme inhibitors

3) allosteric control (binding to enzyme not an active site, changing how it works +shape)

4) temperature and pH

38
Q

enzyme and substrate concentrations

A

1) low enzyme concentration
- reaction rate slows
- enzymes and substrates collide infrequently
(linear, more proportional)

2) high enzyme concentrations
- enzymes become saturated with reactants
- rate of reaction levels off
(levels off, saturation point, enzyme binding sites are occupied and adding more substrate doesn’t affect rate of reaction)

39
Q

enzyme inhibition

A

substances that slow down or stop enzymes from doing their job by either blocking the active site or binding somewhere else on enzyme

COMPETITIVE INHIBITORS
- inhibitor competes with normal substrate for active site

NONCOMPETITIVE INHIBITORS
- inhibitor doesn’t compete with normal substrate for active site, binds somewhere else

can be reversible or irreversible

40
Q

Example of irreversible competitive inhibitor

A

penicillin: antibiotic
- inhibits enzyme (NEED SLIDE)

41
Q

Futile cycle

A
  • futile cycle:
    two metabolic pathways run simultaneously in opposite directions
    NO overall effect: waste of energy
42
Q

Allosteric regulation

A

occurs with reversible binding to the allosteric site (outside of active site on the enzyme)

  • high affinity: enzyme binds strongly (INCREASES RCN RATE)
  • low affinity: enzyme binds weakly or not at all (LOWERS RCN RATE)
43
Q

feedback inhibition

A
  • product of enzyme catalyzed pathway acts as a regulator of the reaction
  • helps conserve cellular resources
44
Q

temperature and pH effects

A
  • enzyme has optimal pH and temp effects
  • as values fall above and below optimum, reaction rates fall off

pH:
- changes in pH affect the charged groups in a.a. of enzyme

temperature:
- temp increases, rate of rxn increases
- gets too high: denatures proteins, and reduces the rate of rxn by doing so

45
Q

What is the second law of thermodynamics

A
  • systems naturally progress towards increased entropy (disorder),
  • meaning that energy tends to spread out and become less usable over time.
  • Spontaneous reactions generally release energy (negative enthalpy) and increase disorder (positive entropy), which lowers Gibbs Free Energy (ΔG).

In simple terms, the universe favors chaos and energy dispersal.

46
Q

What is the second law of thermodynamics

A
  • systems naturally progress towards increased entropy (disorder),
  • meaning that energy tends to spread out and become less usable over time.
  • Spontaneous reactions generally release energy (negative enthalpy) and increase disorder (positive entropy), which lowers Gibbs Free Energy (ΔG).

In simple terms, the universe favors chaos and energy dispersal.

47
Q

Increased disorder means what for the energy

A

Stable because it has a lesser work capacity

48
Q

How is enzyme activity related to the futile cycle

A

We can regulate the speed to ensure 1 pathway is faster than the other so we aren’t losing cell material

BIOL 1101 (4 decks)

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