(A) For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$:Initial moles: $1$ $0$At equilibrium: $(1-\alpha)$ $2\alpha$Total moles at equilibriu

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$\alpha=\sqrt{\frac{K_p}{K_p+4P}}$

(A) For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$:Initial moles: $1$ $0$At equilibrium: $(1-\alpha)$ $2\alpha$Total moles at equilibrium $= 1-\alpha+2\alpha = 1+\alpha$.Partial pressure of $N_2O_4 = \frac{1-\alpha}{1+\alpha} P$.Partial pressure of $NO_2 = \frac{2\alpha}{1+\alpha} P$.$K_p = \frac{(P_{NO_2})^2}{P_{N_2O_4}} = \frac{(\frac{2\alpha}{1+\alpha} P)^2}{\frac{1-\alpha}{1+\alpha} P} = \frac{4\alpha^2 P}{1-\alpha^2}$.Rearranging for $\alpha$:$K_p(1-\alpha^2) = 4\alpha^2 P$$K_p = \alpha^2(4P + K_p)$$\alpha^2 = \frac{K_p}{4P+K_p}$$\alpha = \sqrt{\frac{K_p}{4P+K_p}}$.

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

Medium

For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the correct relation between degree of dissociation $(\alpha)$ of $N_2O_{4(g)}$ and equilibrium constant,$K_p$ is $(P=$ total pressure of mixture $)$

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A
$\alpha=\sqrt{\frac{K_p}{K_p+4P}}$
B
$\alpha=\frac{K_p}{4+K_p}$
C
$\alpha=\left(\frac{K_p / P}{4+\frac{K_p}{P}}\right)^{\frac{1}{2}}$
D
$\alpha=\left(\frac{K_p}{4+K_p}\right)^{\frac{1}{2}}$

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6-1.Equilibrium (Chemical Equilibrium)

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Degree of dissociation and Vapour density

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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 $\%$)

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At temperature $T$,a compound $AB_{2(g)}$ dissociates according to the reaction $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$ with a degree of dissociation $x$,which is very small compared to unity. The value of $x$ is:

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For the equilibrium $PCl_{5_{(g)}} \rightleftharpoons PCl_{3_{(g)}} + Cl_{2_{(g)}}$,the observed vapour density of the mixture is $80$. Given atomic masses $P = 31$ and $Cl = 35.5$,the degree of dissociation of $PCl_{5_{(g)}}$ is approximately....$\%$

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The vapour density of undecomposed $N_2O_4$ is $46$. When heated,the vapour density decreases to $24.5$ due to its dissociation into $NO_{2(g)}$. The percentage dissociation of $N_2O_4$ is:

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$AB_{3(g)}$ dissociates as:
$AB_{3(g)} \rightleftharpoons AB_{2(g)} + \frac{1}{2} B_{2(g)}$. When the initial pressure of $AB_3$ is $800 \ torr$ and the total pressure developed at equilibrium is $900 \ torr$,what percentage of $AB_{3(g)}$ is dissociated?

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For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the correct relation between degree of dissociation $(\alpha)$ of $N_2O_{4(g)}$ and equilibrium constant,$K_p$ is $(P=$ total pressure of mixture $)$

Similar Questions

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 $\%$)

At temperature $T$,a compound $AB_{2(g)}$ dissociates according to the reaction $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$ with a degree of dissociation $x$,which is very small compared to unity. The value of $x$ is:

For the equilibrium $PCl_{5_{(g)}} \rightleftharpoons PCl_{3_{(g)}} + Cl_{2_{(g)}}$,the observed vapour density of the mixture is $80$. Given atomic masses $P = 31$ and $Cl = 35.5$,the degree of dissociation of $PCl_{5_{(g)}}$ is approximately....$\%$

The vapour density of undecomposed $N_2O_4$ is $46$. When heated,the vapour density decreases to $24.5$ due to its dissociation into $NO_{2(g)}$. The percentage dissociation of $N_2O_4$ is:

$AB_{3(g)}$ dissociates as:$AB_{3(g)} \rightleftharpoons AB_{2(g)} + \frac{1}{2} B_{2(g)}$. When the initial pressure of $AB_3$ is $800 \ torr$ and the total pressure developed at equilibrium is $900 \ torr$,what percentage of $AB_{3(g)}$ is dissociated?

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$AB_{3(g)}$ dissociates as:
$AB_{3(g)} \rightleftharpoons AB_{2(g)} + \frac{1}{2} B_{2(g)}$. When the initial pressure of $AB_3$ is $800 \ torr$ and the total pressure developed at equilibrium is $900 \ torr$,what percentage of $AB_{3(g)}$ is dissociated?