a2. reversible, closed
b. When the rate of the forward reaction = rate of backward reaction
c1) All reactant and product species are in the reaction bucket in a reversible reaction wheres in an irreversible reactions there is only products left in reaction bucket (assuming stoichiometric amounts).
c2) Dynamic equilibrium instead of simply Equilibrium emphasizes the concept of even though outwardly or macroscopically there is no change after equilibrium (due to [ ] of all species are constant over time), in reality, both the forward and backward reaction are going but just at same rate.
Why same rate? The product particles are colliding effectively generating Gibb Free Energy so that the reactants that are colliding can make effective collision (remember it needs activation energy). That is why the rate of backward reaction must equal the rate of the forward reaction.
c3) Irreversible reactions, the rearrangement of atoms from reactant to products finishes before the Free Energy different between reactant and products goes to zero. Reversible reaction are the reverse where the Gibbs Free Energy different goes to zero before all the reactants have arranged to products. (why you have both reactants and products are in reaction bucket at equilibrium.
d) Chem rxn and Temp
e) Set of equilibrium concentration of all the species in the bucket
f) more product
g) K = [O2(g)]E3
h1. Reversible reaction in a closed system.
h2. Time independent
h3. Concentration of all reactant and products are constant over time because the rate of the forward and backward reactions are equal.
ia. If you stress an equilibrium system, the system will try to get rid of the stress to go back to the original equilibrium.
ib1) system can only perform the forward reaction or backward reaction
ib2) System can never go back to original equilibrium (because it has different amount of energy/matter/both) so it creates a new equilibrium
ib3) Only substance or attributes (use of energy term for temp and use of number of particles for pressure, determine by adding all coefficients of reactant and same for product) can shift the equilibrium.
j. Decrease Temp (remove/consume Energy), system will make more energy (decrease temp), make more product, favor forward rxn (exothermic), shift Equil to R
k. Increase Pressure (add particles), system decrease pressure (consume particle), make more reactant (3 product particles to 2 reactant praticles), favor backward rxn, shift Equil to L
L. Can either say a) Stress: add OH1-= adding H2O, Rxn: consume H2O, make more reactant, favor backward reaction, shift equilibrium to Left causing solution to get more Yellow.
b) Stress: add OH1- = removing/consuming H3O1+, Rxn: make H3O1+, make more reactant, favor backward reaction, shift equilibrium to Left causing solution to get more Yellow. (Lab condition will not be on section test unless give you all reactions.).
m. 1.67M-2
n. 1.66M
o. 11.9M-1