Kp for the following reaction is 0.16 at 25°C.
2 NOBr(g) (reverse reaction arrow-> <-) 2 NO(g) + Br2(g)
What happens when you decrease and increase volume?
Decreasing volume means pressure is increased; rxn shifts to side with smaller number of moles.
When the volume is decreased, the pressure of the system increases. According to Le Chatelier's principle, a system will shift in a direction that opposes the change. In this case, since the reverse reaction arrow is more product-favored, the system will shift towards the left to decrease the pressure. This means that the concentration of NO, Br2, and NOBr will decrease, while the concentration of NOBr will increase.
Conversely, when the volume is increased, the pressure of the system decreases. Again, according to Le Chatelier's principle, the system will shift in a direction that opposes the change. In this case, the system will shift towards the right to increase the pressure. As a result, the concentration of NO, Br2, and NOBr will increase, while the concentration of NOBr will decrease.
Note that changes in volume only affect the equilibrium position if there is a difference in the stoichiometric coefficients of the gaseous reactants and products. In the given reaction, since the coefficients are the same, changes in volume will only affect the concentrations of the species involved, but not the equilibrium position.