At temperature T,the dissociation equilibrium | vedclass

Name: Exam Paper Generator | JEE NEET Paper Generator | Vedclass
Brand: Vedclass
Rating: 5 (35 reviews)

Question

(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

Vedclass · Accepted Answer

$Px^3 / 2$

Vedclass · Answer

(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}$

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

The vapour density of a mixture containing $NO_2$ and $N_2O_4$ is $27.6$. The mole fraction of $N_2O_4$ in the mixture is

For the equilibrium reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the value of $K_p$ is $2$. Calculate the percentage dissociation of $N_2O_{4(g)}$ at a total pressure of $0.5 \ atm$. (in $\%$)

The degree of dissociation of a weak acid is $7.2 \times 10^{-4}$. What is the value of its percent dissociation in a $0.025 \ M$ solution (in $\%$)?

For the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2NO_{(g)}$; if $K_C = 2$,then the degree of dissociation of $O_2$ is:

$A$ mixture of $NO_2$ and $N_2O_4$ has a vapour density of $38.3$ at $300 \ K$. What is the number of moles of $NO_2$ in $100 \ g$ of the mixture?

Vedclass Test Series

Exam Paper Generator

Online Exam Module