Chapter 1 Flashcards
What four elements make up the majority of the human body?
Carbon
Nitrogen
Oxygen
Hydrogen
What is a condensation reaction?
A reaction that releases water to form two molecules into one
What is a hydrolysis reaction?
A reaction that uses water to break a molecule into two smaller molecules
What is the monomer of protein?
Amino Acid
What is the monomer of nucleic acid?
Nucleotide
What is the monomer of complex carbohydrates?
Monosaccharides (simple carbohydrates)
What major biomolecule does not form polymers?
Lipids
What do enzymes not work on?
Unfavored reactions; because they do not thermodynamically change the reaction
What does the first law of thermodynamics state?
Energy cannot be created nor destroyed but can change form and/or location
What is enthalphy?
Total heat content
When is a reaction exothermic?
When ΔH is negative and it releases energy
When is a reaction endothermic?
When ΔH is positive and it absorbs energy
When is a reaction isothermic?
When ΔH = 0
If a reaction is exothermic, what does it do to energy?
Releases
If a reaction is endothermic, what does it do to energy?
Absorbs
What does the second law of thermodynamics state?
Disorder of the universe always increases
How will systems arrange themself?
To gain freedom and lose restriction
What is entropy?
measure of the disorder in a system
What entropy does an ordered state have?
Low entropy
What entropy does a disordered state have?
High entropy
What does a negative ΔS mean?
The system loses freedom
What does a positive ΔS mean
The system gains freedom
What does Gibbs Free Energy show?
Whether a reaction will occur
What is the equation for ΔG at a constant pressure and temperature?
ΔG = ΔH - TΔS
How do enzymes affect Gibbs’s free energy?
Doesn’t change due to enzymes not affecting the thermodynamics of the reaction
What does a negative ΔG tell us?
Reaction is spontaneous and exergonic (releases energy)
What does a positive ΔG tell us?
Reaction is nonspontaneous and endergonic (absorbs energy)
What does a ΔG = 0 tell us?
Reaction is at equilibrium
What is the ΔG if a reaction is spontaneous?
Negative
What is the ΔG if a reaction is nonspontanous?
Positive
What is the result of a reaction with the following conditions:
ΔH = -
ΔS = +
The reaction is both enthalpically favored (exothermic) and entropically favored. It is spontaneous (exergonic) at all temperatures.
What is the result of a reaction with the following conditions:
ΔH = -
ΔS = -
The reaction is enthalpically favored but entropically opposed. It is spontaneous only at temperatures below T = ΔH/ΔS
What is the result of a reaction with the following conditions:
ΔH = +
ΔS = +
The reaction is enthalpically opposed (endothermic) but entropically favored. It is spontaneous only at temperatures above T = ΔH/ΔS
What is the result of a reaction with the following conditions:
ΔH = +
ΔS = -
The reaction is both enthalpically and entropically opposed. It is nonspontaneous (endergonic) at all temperatures.
What are the standard conditions for ΔGº?
25º C
1 atm
[solutes] = 1.0M
What is the equilibrium constant equal to?
[C]^c * [D]^d / [A]^a * [B]^b
What is ΔGº equal to at equilibrium?
ΔGº = -RTln(k)
What is the equation for a Van’t Hoff Plot?
ln(k) = -ΔHº/R (1/T) + ΔSº/R
What do coupled reactions allow for?
Thermodynamically unfavorable reactions that would not occur on their own
