Consider the following equilibrium in a closed container N 2 O 4(g) leftharpoons 2 NO 2(g) At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements hold true regarding the equilibrium constant (Kp) and degree of dissociation (α) ?

Question

Consider the following equilibrium in a closed container N 2 O 4(g) leftharpoons 2 NO 2(g) At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements hold true regarding the equilibrium constant (Kp) and degree of dissociation (α) ? (A) Neither Kp nor α changes (B) Both Kp and α changes (C) Kp changes but α does not change (D) Kp does not change but α changes

Tardigrade Admin · Accepted Answer

<img class="img-fluid question-image" alt="image" src="https://cdn.tardigrade.in/img/question/chemistry/479deacc60a1ce1092e943b8bf3abd0d-.png" /> At constant temperature, having the volume will change both p and α but Kp remains constant.

Neither $K_{p}$ nor $α$ changes

Both $K_{p}$ and $α$ changes

$K_{p}$ changes but $α$ does not change

$K_{p}$ does not change but $α$ changes

At constant temperature, having the volume will change both $p$ and $α$ but $K_{p}$ remains constant.

Q. Consider the following equilibrium in a closed container N2​O4​(g)⇌2NO2​(g) At a fixed temperature, the volume of the reaction container is halved. For this change, which of the following statements hold true regarding the equilibrium constant (Kp​) and degree of dissociation (α) ?

Neither Kp​ nor α changes

Both Kp​ and α changes

Kp​ changes but α does not change

Kp​ does not change but α changes

At constant temperature, having the volume will change both p and α but Kp​ remains constant.

Neither $K_{p}$ nor $α$ changes

Both $K_{p}$ and $α$ changes

$K_{p}$ changes but $α$ does not change

$K_{p}$ does not change but $α$ changes

At constant temperature, having the volume will change both $p$ and $α$ but $K_{p}$ remains constant.