Chemical Equilibrium Flashcards
Define rate.
the speed at which a process occurs
Define chemical equilibrium.
when the forward and reverse reactions reach a state of balance in which the concentrations of the reactants and products remain the same
Define complex ion.
any metal atom or ion that is bonded to more than 1 atom or molecule
Define ligands.
molecules or anions that readily bond to metal ions
Define solubility product constants.
equilibrium constants for the dissolution of slightly soluble salts
What do reversible reactions do?
They reach equilibrium when the concentration of the reactants and the product is constant
Define Keq.
a constant which shows the ratio of product concentrations to reactant concentrations, with each concentration raised to the power equal to its coefficient at equilibrium
What is a favorable reaction?
A reaction that will have a higher concentration of products than reactants, resulting in a large Keq at equilibrium
Define stress.
something that causes a change in a system at equilibrium
Define Le Chatelierś Principle.
States that when a system at equilibrium is disrupted, the system adjusts in a way to reduce the change
The equilibrium constant is
concentrations of products vs reactants at equilibrium
which of the following can change an equilibrium constant: concentration, rate, temperature, or pressure
temperature
reactions tend to run to completion if
a gaseous product escapes or a precipitate forms
Keq > 1 (large equilibrium constant)
products are favored at equilibrium
Keq < 1 (small equilibrium constant)
reactants are favored at equilibrium
what happens at equilibrium?
both the forward reaction and backward reaction have the same rate
a ligand is a molecule or ion that can
make a bond with a transition metal ion
what must a ligand have?
a lone pair of electrons
at equilibrium…
the concentration of reactants and products must be constant
increasing temperature in an exothermic reaction will shift the equilibrium towards the
products (the right)
Any change in temperature, concentration, or pressure on the system at equilibrium is called a
stress
Which change would shift the equilibrium to the right? N2(g) + 3H2(g) –> 2NH3 (g) + heat: increase the pressure, increase the temperature, decrease the H2, decrease the N2
increase the pressure
If the reactant is added (adding a reactant or removing a product)
the equilibrium shifts to the right
if the product is added (adding a product or removing a reactant)
equilibrium shifts to the left
The Common Ion Effect is used to explain what?
Shift in equilibrium position due to a concentration of an ion
The smaller the value of the solubility product constant:
the lower the solubility of the compound
what can Ksp be applied to?
slightly soluble solutions
Define the Haber process.
The manufacturing of ammonia from nitrogen and hydrogen
Define the common ion effect.
the lowering of solubility of a substance by the presence of a common ion
When do you see a reversible reaction?
when the reaction goes forward and backwards w/o extra energy being used
What happens when you increase pressure at equilibrium?
there is more stress on the high volume than the low volume (pressure will shift to the lower side)
What happens when you decrease pressure at equilibrium?
the reaction proceeds in the direction that raises pressure to where it was (most gas molecules)
What happens when heat is added?
endothermic reaction is favored (shifting to the left, favoring reverse reaction)
What happens when you raise the temperature?
the reaction goes to the right
What happens when you lower the temperature?
reaction goes to the left
