1.Describe and explain a situation in which a soft drink is in a non-equilibrium state.
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I don't really know this question...would a soft dirnk bottle that is opened be a system not at equilibrium...?! When a soft drink bottle is opened, would CO2(g)->CO2(aq) be favoured or CO2(aq)->CO2(g) be favoured? Would there be more gas produced in open bottle or closed bottle?
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2.A series of experiments with a non-aqueous solvent determined that the products are highly favoured in each of the following acid-base equilibria.
(C6H5)3C- + C4H4NH <-> (C6H5)3CH+ C4H4N-
HC2H3O2 + HS- <-> H2S + C2H3O2-
O2- + (C6H5)3CH <-> (C6H5)3C- + OH-
C4H4N- + H2S <-> C4H4NH + HS-
Arrange the acids in the 4 chem. rxns in order of decreasing acid strength.
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I am completely lost...I identified the B-L acids and conjugate pairs...but I have no idea how to which one is stronger!

I have to understand these before the test...I need *delete me* Please teach me! Thank you so much!

H2CO3 <-> H2O + CO2(g)
In a closed bottle it is at equilibrium since the CO2 gas cannot escape.
In an open bottle, the gas escapes, driving the reaction to the right to a non equilibrium.

2) First, for each rxn determine which acid in the pair is more acidic
 C4H4NH > (C6H5)3CH because it is donating H+ to form product on right.
 HC2H3O2 > H2S
etc
etc

Then arrange them all in one series

 There is one acid on each side of the equation. If the acid on the right is stronger, the reaction would go left and vice versa.
You are told the reactions all go to the right.

I already told you in a previous message:
"First, for each rxn determine which acid in the pair is more acidic"

"Then arrange them all in one series "

By using Logic.

correct. Now put them all in one sequence.

"I seeee!" said the blind man.