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increasing the concentration of N2O4 would push the reaction to the right so I think that's out
so d is wrong also
|dw:1439931673570:dw| Increasing the volume though would decrease the pressure and that means that the reaction is going to favor the side with the greater number of moles which is the product so that's out too.
so c is left and correct
In order to reach an equilibrium if you decrease the concentration of the NO2 it's going to want to increased he concentration to achieve equilibrium again so that would go to products
so decreasing the temperature would be rigt
wait.. it's endothermic increasing temperature would favor products but decreasing temp would favor reactants.
If you decrease the concentration of the products when the reaction had already achieved equilibrium it's going to want to achieve equilibrium again since the decrease in concentration kicked it out of its equilibrium. In order for the products to achieve the equilibrium they want to increase the concentration, the increase in concentration will allow the reaction to achieve its equilibrium back. The increase in concentration for the products occurs when more products get made so therefore the forward reaction, so the shift to the right will occur
so.. it's under the assumption that the reaction was already at equilibrium. the decreased concentration of product disrupted equilibrium.
so something is being removed..say a product, that pushes the reaction to the right
Ya I just assumed that it was at equilibrium because it didn't say anything to contradict that possibility If you remove product the reaction proceeds in forward direction If you remove reactant the reaction proceeds in the reverse direction
Thank you tara, my brain hurts so I have to go lol
No problem go have a rest you deserve it!