Quantifying metabolic rxts (Gibbs free energy)

Anabolic

build up, requires energy

(Dehydration synthesis)

Catabolic

break down, releases energy

(Hydrolysis)

Energonic

require energy input, non-spontaneous, small→large

Anabolic

Dehydration synth

Positive G

Energy of products>reactants

Photosynthesis

Exergonic

release energy, spontaneous, large→small
Catabolic
Hydrolysis
Negative G

Energy of products<reactants

Respiration

Delta (triangle)

Final-initial

Gibbs Free Energy formula

ΔG=ΔH-TΔS

H-Enthalpy in KJ

S-entropy in J/K

T is temp

Standard temp is 298 K (25C)

Convert entropy to kj by diving by 1000

Enthalpy

change in heat content

H

Positive during anabolic, negative during catabolic

Entropy

S, joules per kelvin

Measure of amount of disordered in a system

Increases in any system in the absence of an input of energy.

Positive during catabolic reactions, negative during anabolic

-G

more likely to proceed spontaneously

Catabolic

Exergenic

+G

Nonsponateous, anabolic, endergonic

F to K

F=9/5C + 32

C+273=K

First law of thermodynamics

energy is not created or destroyed,only changes forms

Second law of thermodynamics

The sum of entropies of a system and its surroundings must always increase

Which has higher entropy-liquid or solid

Liquid because energy is more dispersed and less orderly.

Third law of thermodynamics

A perfectly crystalline solid at absolute zero has an entropy of zero

Micelle

A structure formed when phospholipids join solution, with hydrophilic heads facing outward and hydrophobic tails inward. Soap,

What are the conditions of S & H (negative/positive) and T (high/low) that lead to spontaneous reactions?What are the conditions of S & H (negative/positive) and T (high/low) that lead to spontaneous reactions?

-H and +S is always spontaneous,

temperatures.

What are the conditions of S & H (negative/positive) and T (high/low) that will not lead to spontaneous reactions?

+H and -S is not spontaneous, -H and -S is not spontaneous at high temperatures, and +H and +S is not spontaneous at low temperatures