Thermodynamics Flashcards

1
Q

a reaction that releases heat is

A

exothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

a reaction that absorbs heat is

A

endothermic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

when H is negative

A

its exothermic - spontaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

when H is positive

A

it’s endothermic - non-spontaneois

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Reactions that increase entropy (+S) tend to be
______

A

spontaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

reactions that release heat (-ΔH) tend to be

A

spontaneous

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

measures the energy difference between the products and reactants and takes into account both entropy and enthalpy

A

gibbs free energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

H stands for

A

Enthalpy change =
heat absorbed or
released

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

T stands for

A

Temperature

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

S stands for

A

enthalpy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

A negative ΔG =

A

spontaneous reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

A positive ΔG =

A

a nonspontaneous reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

(-) ΔG

A

exergonic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

(+) ΔG

A

endergonic

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

what is G dependent on?

A

temperature, pH, relative concentrations of products and reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Standard Gibbs free energy is calculated at ____ (room
temperature), at a pH of __, at __ M of each reactant and
product -> ΔGo

A

Standard Gibbs free energy is calculated at 298 K (room
temperature), at a pH of 7, at 1 M of each reactant and
product à ΔGo

17
Q

The following is the first reaction of glycolysis:
§ Glucose + Pi Glucose-6-phosphate
* ΔGoʼ = 12 kJ/mol
Note the positive ΔGoʼ
How is it possible that a reaction with a
(+) ΔGoʼstill occurs in our bodies – all the
time?

A

This is the whole “rationale” for why the body
phosphorylates ATP (and dephosphorylates it) as a
source of energy currency

  • The high-energy phosphodiester bond, when broken,
    has a negative ΔG
  • That energy can be coupled to another reaction with a
    positive ΔG
  • The net reaction is exergonic…
  • if the ΔG of ATP is “negative enough” to counteract
    the endergonic ΔG of the coupled reaction