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mcat biochem textbook > ch 3 > Flashcards

ch 3 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
what tells you the rate of a rxn? does delta G tell you anything about the rate?
kinetics NOT THERMODYNAMICS, no it does not, it does not depend on rate ONLY difference bw products and reactants
26
what state do all reactions go through and what is the quantity to get there
transition state and the energy to produce a transition state is called the activation energy
27
high Ea means? low Ea?
high Ea means it needs more energy for the rxn to occur vice versa
28
what is a catalyst? what is a biological catalyst
it lowers the Ea without affecting delta G (spon vs nonpon) AND does not get consumed, enzymes
29
photoautotrophs vs chemoheterotrophs
photo=light auto=makes food on own and chemo= eats hetero=doesnt make own food
30
oxidation
lost electrons, loss of H, gain of oxygen
31
reduction
gain of electrons, gain of H, loss of oxygen
32
what is a redox rxn
when something gets oxidized, something else always get reduced
33
catabolism and example
breaking down molecules , glycolysis
34
anabolism and example
building up molecules, glycogenesis
35
what is bronsted lowry acid? lewis acid?
Bronsted Lowry: h+ donor Lewis: electron acceptor
36
what is bronsted lowry base? lewis base?
Bronsted Lowry: h+ acceptor Lewis: electron donor
37
what is a conjugate acid
conjugate acid is formed when a proton is added to a base
38
what is a conjugate base
a acid that has donated its H+ turning it into an base
39
the strength of an acid is based on?
how stable its conjugate base is, and how much it dissociates or not
40
what is Ka
acid dissociation/ionization constant Ka= [H+] [A-]/[HA], high Ka means stronger acid
41
what is Kb
base dissociation/ionization constant Kb= [HB+] [OH-]/[B]
42
amphoteric substance
can act as both an acid or base
43
polyprotic and example
has more than one proton to donate like carbonic acid
44
what is interesting about the conjugate of a polyprotic acid
the conjugate base of a weak polyprotic acid is always amphoteric
45
pH measures what, what are formulas for pH
conc of H+ ions, pH=-log [H+]**** and [H+]= 10^-pH
46
ph>7? ph=7? ph<7?
basic, neutral, acidic
47
pOh measures
conc of OH- ions same formulas pOH=-log[OH-] and [OH-]=10^-pOH
48
if you have pH and pOH what can you do
pH and pOH should equal 14 pH+pOH=14
49
pKa high? low?
high pKa is a weaker acid, low pKA is a strong acid, p usually means -log of something
50
buffer solution
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
what is an important buffer system in our body
bicarbonate H2CO3--> H+ + HCO3-
52
how is carbonic acid created
when our cells produce CO2 as a byproduct, it reacts with water and becomes H2CO3, CO2+ H2O= H2CO3
53
what occurs if you add lactic acid to the bicarbonate buffer solution
low pH occurs and H2CO3 -> H+ +HCO3- moves to the left to increase pH, more base is made
54
if delta g of a reaction is + in one direction
its reverse reaction delta g is - and vice versa
55
Q>K
favors the reverse reaction, more product present
56
Q
favors the forward reaction, more reactant present
57
Q=K
you're in equilibrium
58
what is the third law of TD
a perfect crystal at zero kelvin has zero entropy

mcat biochem textbook (6 decks)

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