change in concentration per unit time

average rate of reaction

rate of change over a period in time

particles must collide with one another in order to react and have sufficent energy for a effective collision

Minimum energy that colliding particles must have for an effective collision to occur.

what factors affect rate of reaction

Nature of reactants Particle size Concentration Temperature Catalysts Pressure (for all-gaseous reaction)

how does temperature affect ROR

increased temperature,particles have increased kinetic energy which means particles reach activation enrergy quicker

how does concentration affect ROR

The more particles the greater the chance of there being an effective collision per unit time.

a substance that alters the rate of reaction without being used up in the process

how do catalysts work

increase the rate of reaction by providing an alternative pathway with a lower activation energy

Are ionic bonds fast or slow to break

generally fast as there is no bond breaking or forming

Are covalent bonds fast or slow to break

slower as bonds need to be broken before a reaction could take place

Reactants adsorbed onto the surface of the catalyst in the correct orientation and in high concentration. Temporary weak bonds form between the reactant and the catalyst There is a high concentration of reactant

The products leave the surface of the catalyst

Heterogeneous Catalysis

The reactant(s) and catalyst are in different phases

Intermediate formation theory of catalysis

Pink at the beginning of the reaction - colour of the catalyst (Co2+) solution. Bubbling and gas are produced as reaction mixture turns green due to formation of intermediate complex.

Limitations of the collision theory Orientation

Particles must collide in the correct orientation for a reaction to occur but it makes it less accurate at predicting rates of reactions involving complex molecules.

Limitations of the collision theory 2. Catalysts

Saturation of catalysts If the surface of the catalyst is fully occupied by the reactant molecules, increasing the concentration will have no effect on the rate of reaction

Limitations of the collision theory 3. Concentration

Limiting reagents: When a reaction involves multiple reactants, an increase in the concentration of one reactant may not alter the rate of reaction unless there is a sufficient amount of the other reactants also present.

what is a reaction profile diagram

Graph that shows the change in energy of a chemical reaction with time as the reaction progresses.

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chem)16)Rate of reac

Question	Answer
rate of reaction	change in concentration per unit time
average rate of reaction	rate of change over a period in time
collision theory	particles must collide with one another in order to react and have sufficent energy for a effective collision
activation energy?	Minimum energy that colliding particles must have for an effective collision to occur.
what factors affect rate of reaction	Nature of reactants Particle size Concentration Temperature Catalysts Pressure (for all-gaseous reaction)
how does temperature affect ROR	increased temperature,particles have increased kinetic energy which means particles reach activation enrergy quicker
how does concentration affect ROR	The more particles the greater the chance of there being an effective collision per unit time.
what is a catalyst	a substance that alters the rate of reaction without being used up in the process
how do catalysts work	increase the rate of reaction by providing an alternative pathway with a lower activation energy
Are ionic bonds fast or slow to break	generally fast as there is no bond breaking or forming
Are covalent bonds fast or slow to break	slower as bonds need to be broken before a reaction could take place
Adsorption	Reactants adsorbed onto the surface of the catalyst in the correct orientation and in high concentration. Temporary weak bonds form between the reactant and the catalyst There is a high concentration of reactant
desorption	The products leave the surface of the catalyst
Heterogeneous Catalysis	The reactant(s) and catalyst are in different phases
Intermediate formation theory of catalysis	Pink at the beginning of the reaction - colour of the catalyst (Co2+) solution. Bubbling and gas are produced as reaction mixture turns green due to formation of intermediate complex.
Limitations of the collision theory Orientation	Particles must collide in the correct orientation for a reaction to occur but it makes it less accurate at predicting rates of reactions involving complex molecules.
Limitations of the collision theory 2. Catalysts	Saturation of catalysts If the surface of the catalyst is fully occupied by the reactant molecules, increasing the concentration will have no effect on the rate of reaction
Limitations of the collision theory 3. Concentration	Limiting reagents: When a reaction involves multiple reactants, an increase in the concentration of one reactant may not alter the rate of reaction unless there is a sufficient amount of the other reactants also present.
what is a reaction profile diagram	Graph that shows the change in energy of a chemical reaction with time as the reaction progresses.

Created by: jp123456789

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