Reading...
Play button
Play button
Use LEFT and RIGHT arrow keys to navigate between flashcards;
Use UP and DOWN arrow keys to flip the card;
H to show hint;
A reads text to speech;
38 Cards in this Set
- Front
- Back
|
H₂0 is what percentage of your wet body weight?
|
70%
|
|
|
What are the 4 major macromolecules of the human body?
|
Carbohydrates
Proteins Nucleic Acids Lipids |
|
|
What 4 atoms make up 87% of human body dry weight?
|
Carbon
Oxygen Hydrogen Nitrogen |
|
|
What 8 atoms make up 97% of human body dry weight?
|
Carbon
Oxygen Hydrogen Nitrogen Potassium Calcium Phosphorus Sulfur |
|
|
How old is life?
|
3400 million years old.
|
|
|
What are the 4 simple steps/stages for chemical evolution?
|
Prebiotic World (H₂O, N₂, CO₂, CH₄ (NH₃, SO₂) ---------->
Organic Molecules ----------> Replicating Molecules ----------> Simple Organisms |
|
|
What elements/molecules (6 of em) were predominant in the Prebiotic World?
|
H₂O, N₂, CO₂, CH₄ (NH₃, SO₂)
|
|
|
Describe the Miller Urey experiment.
- What products did they put in? - What products did they get out? |
Done in the 1953.
Experiment: Subjected a mixture of H₂O, CH₄, NH₃, and H₂ to electric discharges for a week. Result: CO, CO₂, Amino Acids, and Aldehydes. |
|
|
Describe Oparin and Haldane hypothesis about the evolution of biological molecules.
|
Made in the 1930's.
They suggested that UV light from the sun or lightning caused reactions to create organic molecules. |
|
|
What two types of complementarity are required for self-replicating systems?
|
Geometric
Chemical |
|
|
What are the 3 main shapes for Prokaryotic cells?
|
Cocci (round shaped)
Bacilli (oval shaped) Spirilla (spiral shaped) |
|
|
What are the 4 rules for evolution?
|
It is not "goal" oriented.
Requires sloppiness Constrained by the past Ongoing |
|
|
What are the 3 types of energy systems, and what can they transfer?
|
Open System - Everything can be exchanged.
Closed System - Can only exchange energy Isolated System - No energy or matter exchanged. |
|
|
Define:
1'st Law of Thermodynamics |
Energy cannot be created or destroyed.
Internal energy can be changed by exchanging with surroundings. |
|
|
Define:
Entropy |
A measure of randomness (disorder) in a system
|
|
|
Define:
2'nd Law of Thermodynamics |
Spontaneous processes lead to an increase in disorder.
|
|
|
Spontaneous processes/Gibbs Free Energy are represented by the variable...
|
ΔG
|
|
|
Gibbs Free Energy:
If ΔG < 0 ... |
The reaction is exergonic (energy releasing).
The reaction is spontaneous |
|
|
Gibbs Free Energy:
If ΔG > 0 ... |
The reaction is endergonic (energy requiring).
The reaction is non-spontaneous. |
|
|
Gibbs Free Energy:
If ΔG = 0 ... |
The reaction is at equilibrium.
There is no net change in the reactants and products. |
|
|
Define:
Equilibrium At equilibrium, ΔG = ? |
The rate of the forward reactions is equal to the rate of the reverse reactions.
ΔG = 0 |
|
|
Living organisms are _____ systems.
|
open
|
|
|
Describe what each variable represents in:
ΔG = |
ΔG = ΔH - TΔS
ΔG = Change in Gibbs free energy ΔH = Change in enthalpy ΔS = Change in entropy T = Temperature (in kelvins) |
|
|
ΔG = ΔH - TΔS
ΔH is negative ΔS is positive |
Reaction is spontaneous (exergonic) at all temperatures.
Reaction is enthalpically favored (exothermic). Reaction is entropically favored. |
|
|
ΔG = ΔH - TΔS
ΔH is negative ΔS is negative |
Spontaneous only at temperatures below:
T = ΔH/ΔS i.e. T < ΔH/ΔS Reaction is enthalpically favored (exothermic). Reaction is entropically opposed. |
|
|
ΔG = ΔH - TΔS
ΔH is positive ΔS is positive |
Spontaneous only at temperatures above:
T = ΔH/ΔS i.e. T > ΔH/ΔS Reaction is enthalpically opposed (endothermic). Reaction is entropically favored. |
|
|
ΔG = ΔH - TΔS
ΔH is positive ΔS is negative |
Reaction is non-spontaneous (endergonic) at all temperatures.
Reaction is enthalpically opposed (endothermic). Reaction is entropically opposed. |
|
|
ΔG is positive means (spontaneous/nonspontaneous)?
|
nonspontaneous
|
|
|
ΔG is negative means (spontaneous/nonspontaneous)?
|
spontaneous
|
|
|
Define:
ΔH |
Heat transferred at constant pressure and volume.
|
|
|
Define:
Sublimation |
To change from a solid to a gas
(skips the liquid phase) |
|
|
At equilibrium:
ΔG = |
0
zero nada |
|
|
The equilibrium constant, K_eq is...
|
[C] [D] / [A] [B]
|
|
|
The gas constant (R) is...
|
8.31 J / K*Mol
|
|
|
What is room temperature (in Celsius):
|
25 celsius
|
|
|
To go from Celsius to Kelvin, you:
|
add 273.15
|
|
|
ΔG⁰ is called...
|
Standard State Free Energy
|
|
|
At equilibrium, the ΔG equation turns into...
|
ΔG⁰ = -RT ln(K_eq)
|
