Which situation would not cause the following equilibrium reaction to shift to the right? The forward reaction is endothermic. N2O4 (g) Two arrows stacked

Question

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)

decrease the pressure
increase the volume
add N2O4
increase the temperature

Answer 1

N₂O₄(g) + heat <=> 2NO₂(g) 

Since it is stated that the forward reaction is endothermic, we can write "heat" as a reactant.

 

According to Le Chatelier's Principle:

- A decrease in pressure will shift the reaction to the right because the are more moles of gas on the right (2 vs. 1)

- An increase in volume will shift the reaction to the right because that is the same as decreasing the pressure assuming a constant volume. (see above)

- Adding N₂O₄(g) will shift the reaction to the right 

- Increasing the temperature will shift the reaction to the left because this is the same a an increase in pressure, and since there are more moles of gas on the right, the reaction will shift to the left.  This assumes a constant volume.

 

So, answer would be "increasing the temperature".