(C) For the association reaction: $nA \rightleftharpoons A_n$Initial moles: $1$ (for $A$) and $0$ (for $A_n$)Moles at equilibrium: $(1 - \alpha)$ for

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$i = 1 - \alpha + \frac{\alpha}{n}$

(C) For the association reaction: $nA \rightleftharpoons A_n$Initial moles: $1$ (for $A$) and $0$ (for $A_n$)Moles at equilibrium: $(1 - \alpha)$ for $A$ and $\frac{\alpha}{n}$ for $A_n$Total moles at equilibrium $= 1 - \alpha + \frac{\alpha}{n}$The van't Hoff factor $i$ is defined as the ratio of total moles at equilibrium to the initial moles:$i = \frac{1 - \alpha + \frac{\alpha}{n}}{1} = 1 - \alpha + \frac{\alpha}{n}$

Class 12 Chemistry Solutions Abnormal molecular mass

Easy

$A$ solute $A$ undergoes association in a medium as $nA \rightleftharpoons A_n$. If the degree of association is $\alpha$,then the van't Hoff factor $i$ is given by:

A
$i = 1 - \alpha$
B
$i = 1 + \frac{\alpha}{n}$
C
$i = 1 - \alpha + \frac{\alpha}{n}$
D
$i = 1$

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Abnormal molecular mass

For an aqueous solution of $FeSO_4$, the experimental molecular mass is found to be $80 \ g/mol$. What is the degree of dissociation of the salt?

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The observed and calculated molecular weights of calcium nitrate are $65.6$ and $164$ respectively. The degree of dissociation of calcium nitrate is .......... $\%$.

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$75.2 \ g$ of phenol is added to $1 \ kg$ of solvent. The depression in freezing point is $7 \ K$. If phenol undergoes dimerization,calculate the percentage of association. $(K_f = 14 \ K \ kg \ mol^{-1})$

Medium

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If a $0.01 \ m$ aqueous solution of an electrolyte freezes at $-0.056 \ ^{\circ}C$,calculate the van't Hoff factor $(i)$ for the electrolyte. (Cryoscopic constant of water $K_{f} = 1.86 \ K \ kg \ mol^{-1}$)

MediumMHT CET 2023

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$75.2 \ g$ of $C_6H_5OH$ (phenol) is dissolved in a solvent of $K_f = 14 \ K \ kg \ mol^{-1}$. If the depression in freezing point is $7 \ K$,then find the percentage of phenol that dimerises. (in $\%$)

IIT 2006

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$A$ solute $A$ undergoes association in a medium as $nA \rightleftharpoons A_n$. If the degree of association is $\alpha$,then the van't Hoff factor $i$ is given by:

Similar Questions

For an aqueous solution of $FeSO_4$, the experimental molecular mass is found to be $80 \ g/mol$. What is the degree of dissociation of the salt?

The observed and calculated molecular weights of calcium nitrate are $65.6$ and $164$ respectively. The degree of dissociation of calcium nitrate is .......... $\%$.

$75.2 \ g$ of phenol is added to $1 \ kg$ of solvent. The depression in freezing point is $7 \ K$. If phenol undergoes dimerization,calculate the percentage of association. $(K_f = 14 \ K \ kg \ mol^{-1})$

If a $0.01 \ m$ aqueous solution of an electrolyte freezes at $-0.056 \ ^{\circ}C$,calculate the van't Hoff factor $(i)$ for the electrolyte. (Cryoscopic constant of water $K_{f} = 1.86 \ K \ kg \ mol^{-1}$)

$75.2 \ g$ of $C_6H_5OH$ (phenol) is dissolved in a solvent of $K_f = 14 \ K \ kg \ mol^{-1}$. If the depression in freezing point is $7 \ K$,then find the percentage of phenol that dimerises. (in $\%$)

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