Chapter 15: Chemical Equilibrium Flashcards
will a rxn’s equilibrium shift if you add a noble gas to it at constant volume?
no (because adding extra gas to a constant pressure system does not impact the partial pressures of the reactants or products)
will a rxn’s equilibrium shift if you add a noble gas to it at constant pressure?
yes. adding gas at constant pressure will force the volume to increase, which causes the rxn to shift towards the side that has more moles (of gas)
what does the Law of mass action state????
that if the system is at equilibrium at a given temperature, then the following ratio is a constant: [products]^m / [reactants]^n = Keq that the rate of a chemical reaction is proportional to the masses of the reacting substances. Describes the relationship between the concentration of reactants and the concentration of products when their rxn is at equilibrium
in terms of the equilibrium constant k (not the K from rate law expressions), does increasing K make the rxn to go equilibrium sooner/faster?
no. This particular K does represents the concentration of products relative to reactants, not the speed of the rxn.
does dynamic equilibrium occur in open systems?
no. it occurs in closed systems
what is Chemical equilibrium?
state at which the forward and backward processes of a chemical rxn occur at the same rate Doesn’t change over time unless you change the temp
what does a reaction quotient represent?
Q; represents the ratio between products to reactants in a sln at any point in a rxn process (but it is equal to K when the rxn is in equilibrium)
How large must an equilibrium K be in order for us to conclude that products in its rxn are favored?
equilibrium K must be 1 or bigger
How SMALL must an equilibrium K be in order for us to conclude that reactants in its rxn are favored?
equilibrium K must be smaller than 1
what are the 5 different kinds of K so far?
- the K from rate law expressions (rxn speed)
- the equilibrium constant K from Kforward/Kreverse
- the Kc from [products]/[reactants]
- the Kp from (products)/(reactants)
- the Kw
when does Kc = Kp?
if the delta n = 0
how do you go from pH to concentration in your elementary school calculator?
2nd, LOG, -[M]
what is the difference between a rate law expression (chpt 15) and an equilibrium expression (chpt 16)
rate law expressions can be used to tell you about concentrations at any point in a rxn process. equilibrium expressions can be used to tell you about concentrations at one specific point in the rxn process (namely, the point at which the rxn has achieved equilibrium)
how do you go from concentration to pH in your elementary school calculator?
-log [M]
what does an equilibrium constant represent (with respect to reactant and/or product concentrations)?
Kc; represents the ratio between products to reactants in a sln at equilibrium
