how fast a reactant is used up or a product is formed; change in conc/time
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factors effecting rate
surface area,catalyst,temperature,concentration
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collision theory
2 reacting particles must collide for a reaction to occur. Need sufficient energy to overcome the Ea barrier
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catalyst
changes rate of a chemical reaction without being used up, forms an alternative pathway
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heterogenous catalyst
different physical state than reactants
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homogenous catalyst
same physical state as reactants
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equilibrium
a closed system is isolated from its surroundings, so temperature, pressure and concentration of reactants and products are unaffected
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le chatelier's principle
when a system iin equilibrium is subjected to an external change, the system readjusts itself to minimisse the effect of that change.
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pressure
increase in pressure shifts position to the side with fewer molecules
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concentration
if more products form, shifts to right, if more reactants form, shifts to left
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temperature
increase in temp shifts in the endothermic direction, decrease in temp shifts in the exothermic direction
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equilibrium law and kc
increase in Kc, further the position lies to the right, increase concentration of product to reactants. aA + bB(rev)cC+ dD or Kc= (c)^c (D)^d/(A)^a(B)^b
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boltzmann
no molecules have 0 energy, area under line is equal to the total number of molecules, no maximum energy for a molecule- y axis=no.molecules with sufficient energy, x axis-energy
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increase in temperature
increase in molecules have an energy greater or equal to activation energy therfore there is an icrease in proportion of collisions and an increase in rate.
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