(A) The initial moles are $2$ moles of $AB_2$. Let the degree of dissociation be $x$.For the reaction: $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2

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(A) The initial moles are $2$ moles of $AB_2$. Let the degree of dissociation be $x$.For the reaction: $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$Initial moles: $2, 0, 0$Moles at equilibrium: $2(1-x), 2x, x$Total moles at equilibrium $= 2-2x+2x+x = 2+x$.Partial pressures at equilibrium:$p_{AB_2} = \frac{2(1-x)}{2+x} P \approx P$ (since $x \ll 1$)$p_{AB} = \frac{2x}{2+x} P \approx xP$$p_{B_2} = \frac{x}{2+x} P \approx \frac{x}{2} P$$K_p = \frac{(p_{AB})^2 (p_{B_2})}{(p_{AB_2})^2} = \frac{(xP)^2 (xP/2)}{P^2} = \frac{Px^3}{2}$

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Degree of dissociation and Vapour density

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At temperature $T$,the dissociation equilibrium of $AB_{2(g)}$ is given as: $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$. If the degree of dissociation $x$ is very small compared to $1$,then the expression for the equilibrium constant $K_p$ in terms of $x$ and total pressure $P$ is:

A
$Px^3 / 2$
B
$Px^2 / 3$
C
$Px^3 / 3$
D
$Px^2 / 2$

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6-1.Equilibrium (Chemical Equilibrium)

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Degree of dissociation and Vapour density

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At temperature $T$,the dissociation equilibrium of $AB_{2(g)}$ is given as: $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$. If the degree of dissociation $x$ is very small compared to $1$,then the expression for the equilibrium constant $K_p$ in terms of $x$ and total pressure $P$ is:

Similar Questions

$3.2$ moles of hydrogen iodide were heated in a sealed bulb at $444\,^{\circ}C$ till the equilibrium was reached. The degree of dissociation of $HI$ at this temperature was found to be $22\%$. The number of moles of hydrogen iodide present at equilibrium are

Calculate the degree of dissociation $\alpha$ for $0.1 \, N \, CH_3COOH$ (dissociation constant $K_a = 1 \times 10^{-5}$).

In a $100 \ L$ vessel,$3 \ moles$ of nitrogen and $3 \ moles$ of $PCl_5$ are taken and heated to $500 \ K$. The equilibrium pressure is $3.28 \ atm$. The percentage degree of dissociation of $PCl_5$ is : (Assume ideal behaviour for all gases).

For the reaction $A \rightleftharpoons nB$,if $a$ moles of $A$ are taken initially and $x$ moles of $A$ dissociate at equilibrium,find the value of the degree of dissociation.

For the reaction,$N_2 + O_2 \rightleftharpoons 2NO$,the equilibrium constant is $K_c = 2$. If both reactants have the same initial moles,what is the degree of dissociation of $N_2$ and $O_2$?

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