1.
1st Law of Thermodynamics: Energy can never be created nor destroyed
2.
2nd Law of Thermodynamics: Entropy increases
3.
3rd Law of Thermodynamics: Entropy= 0 at 0 K
4.
A chemical reaction with positive free energy: will proceed in the forward direction if the substrate concentration is raised high enough
5.
A positive DeltaEo results in: negative DeltaGo, exergonic
6.
Adding more reactants will shift the log-log graph: Left
7.
Delta Go: is the standard free energy at 25 degrees C and pH 7
8.
During a heart attack you will have: increased intracellular H+ concentration
9.
Equilibrium: No energy
10.
Exogoneric Reaction: Spontaneous
11.
High reduction potential: electron acceptor
12.
In a log-log plot the delta G is on the: y-axis
13.
In a log-log plot the equilibrium ratio is on the: x-axis
14.
Is this reaction thermodynamicaly favorable? ATP + glucose= glu-6-P + ADP: Yes, Delta Go' is negative overall
15.
K equilibrium < 1: Reaction favors reactants
16.
K equilibrium > 1: Reaction favors products
17.
NAD is: energy poor
18.
NAD+: accepts 2 electrons as a hydride ion to form NADH
19.
NADH is: energy rich
20.
NADH is_________ to NAD+: oxidized
21.
Negative Delta G: favoring products, thermodynamically favorable
22.
Negative Delta H and Negative Delta S: Enthalpically favored and entropically opposed. Spontaneous at temperatures below T= DeltaH/DeltaS.
23.
Negative Delta H and Positive Delta S: Enthalpically and entropically favored. Spontaneous at all temperatures.
24.
oxidation: is loss of electron
25.
Positive Delta G: favoring reactants, not thermodynamically favorable
26.
Positive Delta H and Negative Delta S: Enthalpically and entropically unfavored. Never spontaneous.
27.
Positive Delta H and Positive Delta S: Enthalpically unfavored and entropically favored. Sponteous at temperatures above T= DeltaH/DeltaS
28.
reduction: is gain of electrons
29.
Steady state: Energy
30.
Steady state constant: MAR
31.
The change in enthalpy of a reaction is: the total amount of heat that can be released from changes in the chemical bonds
32.
The change in enthalpy, DeltaH: is the total amount of heat that is released in a reaction
33.
The highest energy phosphate bond in ATP is located between: the 2 phosphates
34.
The more negative the Eo value the: greater the potential to donate electrons
35.
The Nerst equation is used for: oxidation-reduction reactions
36.
Ultimate acceptor of electrons and high reduction potential: oxygen
37.
Why is advantageous for cells to use ATP as their primary energy-carrying molecule?: ATP can be regenerated by coupling with a reaction that releases more free energy than does ATP hydrolysis
