Energy
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- In a local closed system, orderliness can arise without entropy increasing. However, the energy used to maintain this order will be transferred to an unusable form, hence causing entropy to increase outside the system.
- In chemical reactions, entropy increases when
- Solids become liquid/gas products (or liquid becomes gas products)
- x moles of reactant molecules form more than x moles of product molecules
- Complex molecules form simpler molecules
- Solutes diffuse to achieve a homogeneous mixture
- Energy in a reaction
- 1) Activation energy is absorbed by the reactants to break bonds 2) Reactants enter transition state 3) As products form by bonding, energy is released
- Product is more stable (bond energy is higher) than reactants
- Change in Heat energy is negative = Exothermic reaction; Change in heat energy is positive = Endothermic
- Free Energy (usable energy) in a reaction
- Change in Gibbs free energy is negative = Exergonic reaction [spontaneous]; Change in Gibbs free energy is positive = Endergonic reaction [not spontaneous]
- Metabolic Reactions
- ATP + ATPase --> ADP + Pi + Energy
- Energy is usually not released as heat; Instead, it is coupled with an endergonic reaction
- Redox reaction
- Involves oxidation and reduction
- A series of redox reactants result in the final oxidizing agent (that gets reduced) being the strongest
- Reduces activation energy required for a reaction
- Enzymes are inhibited by competitive inhibitors (resembling the substrate) and noncompetitive inhibitors (alters binding site by binding to another site)
- Allosteric sites
- Activators: bind to these sites to stabilize an active form of the enzyme
- Inhibitors: bind to these sites to stabilize an inactive form of the enzyme
- Feedback Inhibition: Substrate --enzyme 1--> Intermediate A --enzyme 2--> Intermediate B --enzyme 3 --> end product...............end product inhibits enzyme 1.
- If end product concentration decreases, less enzyme 1 is inhibited and more end product is produced.