Studied by 3 people
Reversible yield arrows
indicate that the reaction occurs significantly in both directions
Equilibrium is
dynamic; reaction is still happening
K = 1
There are roughly the same amount of both
K > 1
more products
K < 1
more reactants
K < 10^-3
reactants dominate
K > 10³
products dominate
10^-3 < K < 10³
significant amount of both
To determine if in equilibrium
use q and the ICE chart if given initial and equilibrium
Le Chatelier’s principle
if a reaction is disturbed, then it will shift to partially counteract that disturbance
Volume of container is reduced
shift towards fewer moles (less pressure)
net ionic equation
total ionic equation - spectator ions
avogadro’s number; a mole
6.02 × 10 ^ 23
yield percent
actual/theoretical * 100
Note
Flashcard