[ME1987]

Please help I've been trying to figure these questions out and I'm so frustrated  I'm about to cry. I've tried all weekend.  Here they are:How will this equilibrium be affected by the changes listed below?
      N2O4 (g) + energy ? 2NO2 (g)  

a.   The pressure in increased by decreasing the volume.
b.   The pressure in increased by adding NO2.
c.   The pressure is increased by adding N2O2.
         
 
               The following reaction is at equilibrium.
     
      Ba(ClO3)2(s) ? Ba2+(aq) + 2ClO3-(aq)

   Use LeChâtelier’s principle to determine whether the following changes shift the equilibrium to the left or to the right.    
a.   The temperature is increased.
b.   Barium nitrate is added.
c.   More Ba(ClO3)2(s) is added.  

PS. the squares are those arrows.

[Borek]

Show us what you have tried and where are you stuck.

[ME1987]

I don't really know where to start.  That's one of the reasons I'm so frustrated .

[Vette Freak]

What is Le Chatelier's Principle?  Reactions in equilibrium want to stay there so they do everything they can to neutralize any changes.  How can the reaction process shift to counter the changes made to it?  Will it make more reactants or more products?

[lonilonei]

Ok, I think this might be a little late, but anyhow,

Please help I've been trying to figure these questions out and I'm so frustrated  I'm about to cry. I've tried all weekend.  Here they are:How will this equilibrium be affected by the changes listed below?
      N2O4 (g) + energy ? 2NO2 (g)  

a.   The pressure in increased by decreasing the volume.
b.   The pressure in increased by adding NO2.
c.   The pressure is increased by adding N2O2.

Remember that Le Chartier's principle states that the equilibrium will shift to try and counter the effects of a change. So by decreasing volume, the concentrations of all gases are increased, but equilibrium will shift to try and counter this by moving toward the side of the equation with less molcules i.e toward the reactants in teh above case.

For the other two questions, don't see it as adding pressure, see it as incresing the concentration and treat the rest as per normal.    

               The following reaction is at equilibrium.
      
      Ba(ClO3)2(s) ? Ba2+(aq) + 2ClO3-(aq)

   Use LeChâtelier’s principle to determine whether the following changes shift the equilibrium to the left or to the right.     
a.   The temperature is increased.
b.   Barium nitrate is added.
c.   More Ba(ClO3)2(s) is added.  

PS. the squares are those arrows.

Once again, do the same, but this time, remember the tricks of temperature changes. It's strange they haven't told you whether the reaction is endo or exothermic, as this is the key to which way the equilbrium shifts under temperature changes...