rates Flashcards
collision theory
reactant molecules must collide with sufficient energy and the correct orientation for a reaction to occur (bounce off otherwise)
area under curve for maxwell boltzmann distribution
of particles in sample
Ea
minimum amount of energy required for a reaction to occur
ROR key words
PER UNIT TIME
factors affecting ror: fq
surface area
concentration
pressure
factors affecting ror: proportion
temperature
catalyst
increase pressure with equal gas moles
bc equal gas moles, system cannot partially oppose therefore no effect on yield
increase temp favours higher ror bc
particles have more Ke tf collide with more force
when describing ror on graphs talk about
steepness of curves representing ror
improve accuracy of calculating ror by
measure pH
video record and stop video every certain time period
Kc represents
extent of reaction
> 10^4 reaction goes to completion
< 10^-4 reaction negligible extent only
equilibrium =
rate of forward and reverse reaction are equal
le chatellier principle key words
tendency to PARTIALLY OPPOSE change
what effect does adding inert gas have
NO EFFECT
what affects Kc
TEMPERATURE
How to determine theroretical voltage produced by a single cell
(NOT DEPENDENT ON BALANCING NUMBERS)
E(big) - E(small)
what effects pH
ONLY H+ IONS (not OH)
what effects neautrality/ making something acidic/basic
charge/ proportion of OH to H+
You can have a low pH hw the system still be neutral
effect on temperture on Kc value
exothermic: as t increases -> k decreases
endothermic: as t increases -> k increases
rate of reaction
change in concn of a reactant or pruduct per unit time
catalysts
speed up chemical reactions, providing an alternative reaction pathway by lowing activation energy
what does the equilibrium constant measure
the extent of the reaction
what is the K value if the reaction goes to completion
K> 10 ^4
what is the K value if reation occurs to a neglibible extent
K< 10^-4
effect on Kc if equation is reversed
recipical of K
effect on Kc if equation coefficients are doubled
K ^2
effect on K if co-efficients are halved
K ^1/2
effect on dilutions on equilibrium
dilution -> decrease concentration -> favour side with more aqu moles
hw this does not make solution more intense bc already diluted
