In this question, all gases can be assumed to behave ideally. A chemist heats a mixture of nitrogen and oxygen gases in a sealed container at a constant temperature until the mixture reaches a dynamic equilibrium containing N₂(g), O₂(g) and NO(g). N₂(g) + O₂(g) ⇌ 2NO(g) The chemist repeats the experiment at the same temperature using the same initial amounts of N₂(g) and O₂(g), but at a much higher pressure. Which statements about the second experiment at higher pressure are correct? 1 At higher pressure, there are more particles per unit volume. 2 The composition of the equilibrium mixture does not change. 3 There are more collisions per second so equilibrium is reached faster.