Consider the following equilibrium in a closed container: N_(2)O_(4(g))iff2NO_(2(g)) At a fixed temperature, the volume of the reactioncontainer is halved. For this change, which of the following statements, holds true regarding the equilibrium constant (K_(p)) and degree of dissociation (alpha)?

Consider the following equilibrium in a closed container: N_(2)O_(4(g

1.	Consider the following equilibrium in a closed container: N_(2)O_(4(g))iff2NO_(2(g)) At a fixed temperature, the volume of the reactioncontainer is halved. For this change, which of the following statements, holds true regarding the equilibrium constant (K_(p)) and degree of dissociation (alpha)?
Answer» <P>NEITHER `K_(p)` nor `ALPHA` changes Both `K_(p) and alpha` change `K_(p)` changes but `alpha` not change `K_(p)` does not change, but `alpha` changes Solution :`K_(p)` is constant at constant temperature. As VOLUME is halved, PRESSURE will be doubled. Hence equilibrium will shift in the backward direction i.e., degree of dissociation decreases.