Section Two Flashcards
Pressure
Higher pressure Gases have less space between particles Increased number of collisions between particles Increase chance of successful collision Increase rate of reaction
Particle size
Increase surface area
Increase number of collisions between reactants
Increase chance of an successful collision
Increase rate
Temperature
Increase temp Increase energy of particles Increase the number of particles That can get over the activation barrier Increase successful collisions Increase rate
Activation barrier
Minimum energy required for a reaction to occur
Not every collision has enough energy to be successful
Not enough energy
Bounce off each other
No reaction occurs
Fast reaction
Low activation energy (little hill)
Transition state
Only lasts for a fraction of a second
Unstable
Successful reaction
Enough energy
Collide with correct geometry
Catalyst
Chemicals which speed up reactions
Not used up in a reaction
Give the reaction an alternative path
To making the products that require less energy
Biological catalysts
Enzymes made in cells
Speed up the chemical reaction
Lock and key function best in a narrow range of phs
Effect of temperatures on enzymes
On how well enzyme functions
When humans have temperatures
Enzymes don’t function properly
Enthalpy
Given amount of energy
Of reactant chemicals
Hr
Chemical energy
First one
Hp
Energy of the products
Exothermic reactions
Enthalpy is given out or lost
Surroundings become hotter
Energy lost from reactants
Reactants have MORE energy then products
