Which situation would not cause the following equilibrium reaction to shift to the right? The forward reaction is endothermic. N2O4 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NO2 (g) Increase the pressure Increase the volume Increase the concentration of N2O4 Increase the temperature

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Which situation would not cause the following equilibrium reaction to shift to the right? The forward reaction is endothermic. N2O4 (g) Two arrows stacked on top of each other. The top arrow points to the right. The bottom arrow points to the left. 2 NO2 (g) Increase the pressure Increase the volume Increase the concentration of N2O4 Increase the temperature

Chemistry
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d?
Hm, no, it is an endothermic reaction, so heat is a reactant. When you increase a reactant, it pushes the reaction toward the products.

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Other answers:

ahh so c
No, that is again increasing the amount of a reactant.
a?
http://www.chemguide.co.uk/physical/equilibria/lechatelier.html
iget it b is the correct answer
No, b isn't correct. Which side has more molecules?
of gas
left side but a is correct?
Yes, because when you increase the pressure, it is going to shift the reaction toward the side with less gas molecules.
okay

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