equilibrium

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what is the rate of reaction
it measures how fast a reactant is being used used up or how fast a product is being formed
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what is the equation for the rate of reaction
rate = change in conc./time
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how do you explain rate time graphs
the rate of reaction is fastest at the start of the reaction as there is the highest conc. the rate slows as reaction proceeds as reactants being used up the when reactants completely used up the conc. stops changing and rate is zero
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what factors affect the rate of reaction
conc.(pressure in gases)
temperature
use of catalyst
surface area of solid
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What is collision theory
state that two reacting particles must collide result in a chemical reaction
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how must particles collide to form a product
the particles must collide with the correct orientation and have sufficient energy to overcome the activation energy
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what is the method of following a progress of reaction
monitoring the removal of a reactant or following the formation of a product
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what is the reactant is a gas
monitor the gas volume at regular time intervals or monitor the loss of reactants using a balance
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what is an examples of a practical used to collect gas volumes
the decomposition of hydrogen peroxide using a conical flask and a delivery tube or using calcium carbonate and HCl and measuring the mass on a balance at intervals
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what is a catalyst
it is a substance that changes the rate of a chemical reaction with undergoing any permanent change
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what are the two different types of catalyst
homogenous and heterogenous
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what is a homogenous catalyst
it is a catalyst that has the same physical state as the reactants
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what are some examples of reactions with homogenous catalysts
making esters with a sulphuric acid catalyst or ozone depletion cl radical as a catalyst
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what is a heterogenous catalyst
it is catalyst that has a different stat from the reactants
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what are some examples of heterogenous catalysts
making ammonia in the haber process
hydrogenation of alkenes
making sulphur trioxide
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what are some features of boltzmann distribution
no molecules have zero energy - the curve starts at the origin
the are under the curve is equal to the total number of molecules
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what does a boltzmann distribution look like at higher temperatures
more molecules have an energy greater than or equal to the activation energy
greater proportion of collisions will lead to a reaction increasing the rate of reaction and collisions will be more frequent
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what is a dynamic equilibrium
the rate of the forward reaction is equal to the rate of the reverse reaction
the concentrations of reactants and products do not change and must be in a closed system
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what is Le chatliers principle
states that when a system in equilibrium is subjected to an external change the system readjusts itself to minimise the effect of that change
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what is the equation for the rate of reaction

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rate = change in conc./time

Card 3

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how do you explain rate time graphs

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Card 4

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what factors affect the rate of reaction

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What is collision theory

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