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mcat biochem textbook > ch 3 > Flashcards

ch 3 Flashcards

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MCAT flashcards
1
Q

thermodynamics

A

study of energies of chemical rxns

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2
Q

kinetic energy

A

movement of molecules

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3
Q

potential energy

A

energy stored in chemical bonds

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4
Q

first law of TD

A

conservation of energy, the energy of the universe is constant. If energy in the system decreases, the energy in the surrounding universe goes up

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5
Q

second law of TD

A

entropy tends to increase, spontaneous reactions increase disorder and entropy is delta S

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6
Q

gibbs free energy

A

a thermodynamic quantity equal to the enthalpy (of a system or process) minus the product of the entropy and the absolute temperature.

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7
Q

enthalpy

A

total heat constant of a system, calculated by adding change in Energy plus the product of the pressure and change in volume in the system

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8
Q

what are the conditions for an increase in delta G

A

high enthalpy and low entropy, you can see the relationship through the formula

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9
Q

what does change in delta G show

A

whether a rxn is favorable or not

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10
Q

what is - delta G, + delta G?

A
  • delta G is spontaneous or favorable and + delta G is nonspontaneous or unfavorable
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11
Q

spontaneous rxns are (gonic)

A

exergonic (energy released)

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12
Q

nonspontaneous rxns are exogernic or endergonic?

A

endergonic (energy consumed), meaning energy is needed to occur

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13
Q

-delta H is what kind of reaction (thermic?)

A

exothermic (heat released)

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14
Q

+delta H is what kind of reaction (thermic)

A

endothermic (heat consumed)

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15
Q

energy always goes to what energy state

A

towards the lower energy state or the most stable, like how hot things turn cool, spinning top to motionless top

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16
Q

what is the standard delta G? what is the formula

A

where all solutes are 1 Molar except H+ and has a pH of 7.
Delta G is given by -RT In Keq where R is gas constant, Keq is ratio of products to reactants at eq, and T is temp

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17
Q

what is Keq?

A

products over reactants conc at eq.

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18
Q

what is the formula for delta G in the body

A

delta G equals to standard delta G + RT In Q where Q is products over reactants at their true concentrations NOT equilibrium

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19
Q

whats the difference between Keq and Q

A

Keq is products over reactants AT EQUILIBRIUM and Q is products over reactants at any set-up

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20
Q

what is equilibrium

A

where the forward rxn equals the backwards rxn

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21
Q

adding more or less products can affect what

A

the Q but NOT THE Keq

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22
Q

high Keq means

A

more products 10/2= 5

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23
Q

what does Q NOT tell you

A

if the products are high or low, only what the inital conc is

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24
Q

what is delta g of zero mean

A

equilibrium

25
Q

what tells you the rate of a rxn? does delta G tell you anything about the rate?

A

kinetics NOT THERMODYNAMICS, no it does not, it does not depend on rate ONLY difference bw products and reactants

26
Q

what state do all reactions go through and what is the quantity to get there

A

transition state and the energy to produce a transition state is called the activation energy

27
Q

high Ea means? low Ea?

A

high Ea means it needs more energy for the rxn to occur vice versa

28
Q

what is a catalyst? what is a biological catalyst

A

it lowers the Ea without affecting delta G (spon vs nonpon) AND does not get consumed, enzymes

29
Q

photoautotrophs vs chemoheterotrophs

A

photo=light auto=makes food on own and chemo= eats hetero=doesnt make own food

30
Q

oxidation

A

lost electrons, loss of H, gain of oxygen

31
Q

reduction

A

gain of electrons, gain of H, loss of oxygen

32
Q

what is a redox rxn

A

when something gets oxidized, something else always get reduced

33
Q

catabolism and example

A

breaking down molecules , glycolysis

34
Q

anabolism and example

A

building up molecules, glycogenesis

35
Q

what is bronsted lowry acid? lewis acid?

A

Bronsted Lowry: h+ donor Lewis: electron acceptor

36
Q

what is bronsted lowry base? lewis base?

A

Bronsted Lowry: h+ acceptor Lewis: electron donor

37
Q

what is a conjugate acid

A

conjugate acid is formed when a proton is added to a base

38
Q

what is a conjugate base

A

a acid that has donated its H+ turning it into an base

39
Q

the strength of an acid is based on?

A

how stable its conjugate base is, and how much it dissociates or not

40
Q

what is Ka

A

acid dissociation/ionization constant Ka= [H+] [A-]/[HA], high Ka means stronger acid

41
Q

what is Kb

A

base dissociation/ionization constant Kb= [HB+] [OH-]/[B]

42
Q

amphoteric substance

A

can act as both an acid or base

43
Q

polyprotic and example

A

has more than one proton to donate like carbonic acid

44
Q

what is interesting about the conjugate of a polyprotic acid

A

the conjugate base of a weak polyprotic acid is always amphoteric

45
Q

pH measures what, what are formulas for pH

A

conc of H+ ions, pH=-log [H+]** and [H+]= 10^-pH

46
Q

ph>7? ph=7? ph<7?

A

basic, neutral, acidic

47
Q

pOh measures

A

conc of OH- ions same formulas pOH=-log[OH-] and [OH-]=10^-pOH

48
Q

if you have pH and pOH what can you do

A

pH and pOH should equal 14 pH+pOH=14

49
Q

pKa high? low?

A

high pKa is a weaker acid, low pKA is a strong acid, p usually means -log of something

50
Q

buffer solution

A

a solution that resists changes in pH when a small amount of acid or base is added, it has equal parts of weak acid and its conjugate base

51
Q

what is an important buffer system in our body

A

bicarbonate H2CO3–> H+ + HCO3-

52
Q

how is carbonic acid created

A

when our cells produce CO2 as a byproduct, it reacts with water and becomes H2CO3, CO2+ H2O= H2CO3

53
Q

what occurs if you add lactic acid to the bicarbonate buffer solution

A

low pH occurs and H2CO3 -> H+ +HCO3- moves to the left to increase pH, more base is made

54
Q

if delta g of a reaction is + in one direction

A

its reverse reaction delta g is - and vice versa

55
Q

Q>K

A

favors the reverse reaction, more product present

56
Q

Q<K

A

favors the forward reaction, more reactant present

57
Q

Q=K

A

you’re in equilibrium

58
Q

what is the third law of TD

A

a perfect crystal at zero kelvin has zero entropy

mcat biochem textbook (6 decks)

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