STM 006 Flashcards
This inside of theory state that molecules must collide in order to react. And in order to effectively initiate a reaction, collisions must be sufficient energetic to break a chemical bonds.
THE COLLISION THEORY
An area of chemistry that deals how fast chemical reaction occurs and a factor that influence the rate of reaction.
CHEMICAL KINETICS
The theory that state atoms, ions, and molecules must collide.
THE COLLISION THEORY
The collision theory was proposed by two people with different year.
MAX TRAUTZ (1916) AND WILLIAM LEWIS (1918)
A qualitative explanation of chemical reactions and the rates at which they occur. With a basic principal that state, in order to react, molecules must collide.
COLLSION THEORY
Th more molecules present, the more collisions will happen. Low concentration, few collisions and the high concentration the more collisions.
MOLECULAR COLLISION
This minimum energy with which molecules must be moving in order for a collision to result in a chemical reactions and to make the bond break is known as the
ACTIVATION ENERGY
This is a theory that the kinetic energy of gas is directly proportional to temperature. The greater the temperature the higher the probability that molecules can move into activation energy for a reaction to occur upon collision.
THE KNETIC THEORY OF GASES
One in which molecules collide with sufficient energy and proper orientation, so that a reaction occurs.
EFFECTIVE COLLISION
Molecules must collide with sufficient energy, so that the chemical bond break.
ACTIVATION ENERGY
This theory provides an explanation for how particles interact to cause a reaction and formulate a new product.
COLLISION THEORY
This theory provides an explanation for how particles interact to cause a reaction and formulate a new product.
COLLISION THEORY
Increasing the temperature will cause he particles to move faster with more energy. They will collide more often and with greater energy. The faster the reaction.
TEMPERATURE
Increasing the concentration of a reactant simply means there are more particles which may collide and so react. And the more collision the faster the reaction.
CONCENTRATION
When the surface is greater means a greater area of reactants is exposed and so available. More collision the faster the reaction
SURFACE AREA
If they collide only moderate energy, this means more successful collisions are likely .
CATALYS
A chemical reaction that is kind of like that “hump” you have to get over to get your self out of the bed.
ACTIVATION ENRGY
A high-energy state, and some amount of energy the activation energy must be added in order in order for the molecule reach it.
TRANSITION
It state that a reaction is always at a higher energy level than the reactants or products.
TRANSITION
A source that is typically heat, with reactant molecules absorbing thermal energy from their surrounding.
THE SOURCE OF ACTIVATION ENERGY
This is the process at which speeding up a reaction by reducing its activation energy.
CATALYSIS
This is the factor that is added to lower to lower he activation energy.
CATALYST
What is the biological catalyst?
ENZYMES
The speed up a chemical by lowering the amount of energy. The used in making plastics and many other manufactured items. The key of unlocking biofuels
CATALYST
The backbone of many industrial processes. Use chemical reactions to turn raw materials into useful products.
CATALYSIS
Speed up a chemical reaction by lowering
the amount of energy you need to get one
going. A way to save energy
CATALYST
The process of speeding up a reaction by
reducing its activation energy.
CATALYSIS
What are the two main types of catalysts.
HETEREGENOUS AND HOMOGENEOUS
A catalyst reaction that in a different phase from the reactants.
HETEREGENOUS REACTION
A catalyst reaction that in a same phase as the reactants.
HOMOGENOUS REACTION
This the same phase as the reactants
CATALYST
This the space that is you can’t see any boundary between them. Which don’t dissolve in each other, and or you could see the boundary of each other liquids.
PHASE
The one of the reactants on the surface of the catalyst at active sites.
ABSORBED
This is where something is sticks to a surface.
ABSORPTION
When the product molecules break away. This leaves the active site available for a new set of molecule to attached and react.
DESORPTION
The natural proteins (enzyemes) or nucleic acids like (RNA AND DNAs) used to catalyze specific chemical reactions outside the living cells is called
BIOCATALYSIS
The obtain from animals tissue, plants and microbes. A high selective, high efficiency, eco-friendliness and mild reaction condition.
ENZYMES
A laws define the
fundamental physical quantities like energy,
temperature and entropy that characterize. The relationship between thermal energy, or heat and other forms of energy, and how energy affects matter.
Thermodynamic Laws
A one of the law of thermodynamics state that energy cannot be created or destroyed, the total quantity of energy in the universe stays the same.
THE FIRST LAW OF THERMODYNAMICS.
A one of the law of thermodynamics state about the quality of energy, as the energy is transferred or transformed, more and more of it is wasted. There is a natural tendency of any isolated system to degenerate into a more disordered state.
THE SECOND LAW OF THERMODYNAMICS
The degree of randomness in a substance.
ENTROPHY
They both discovered the basis for the second law of thermodynamics.
RUDOLF CLAUSIUS AND WHILIAM THOMSON (LORD KELVIN) AROUND 1850
