(B) The reaction is: $CH_3COOH_{(l)} + C_2H_5OH_{(l)} \rightleftharpoons CH_3COOC_2H_{5(l)} + H_2O_{(l)}$Initial moles: $4 \ mol$ of $CH_3COOH$ and $4

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(B) The reaction is: $CH_3COOH_{(l)} + C_2H_5OH_{(l)} \rightleftharpoons CH_3COOC_2H_{5(l)} + H_2O_{(l)}$Initial moles: $4 \ mol$ of $CH_3COOH$ and $4 \ mol$ of $C_2H_5OH$.Let $x$ be the moles of product formed at equilibrium.Equilibrium moles: $CH_3COOH = (4-x)$,$C_2H_5OH = (4-x)$,$CH_3COOC_2H_5 = x$,$H_2O = x$.$K_c = \frac{[CH_3COOC_2H_5][H_2O]}{[CH_3COOH][C_2H_5OH]} = \frac{x^2}{(4-x)^2} = 4$Taking the square root on both sides: $\frac{x}{4-x} = 2$$x = 8 - 2x$ $\Rightarrow 3x = 8$ $\Rightarrow x = 8/3$Concentration of acid at equilibrium = $4 - x = 4 - 8/3 = 4/3 \ mol$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

Difficult

For the esterification reaction $CH_3COOH_{(l)} + C_2H_5OH_{(l)} \rightleftharpoons CH_3COOC_2H_{5(l)} + H_2O_{(l)}$,the equilibrium constant $K_c$ is $4$. If $4 \ mol$ of each acid and alcohol are taken initially,what will be the concentration of the acid at equilibrium?

A
$2/3$
B
$4/3$
C
$3/4$
D
$3/2$

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6-1.Equilibrium (Chemical Equilibrium)

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Mix Examples- 6-1.Equilibrium (Chemical Equilibrium)

$AB_{3(g)}$ 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 fraction of $AB_{3(g)}$ is dissociated? .....$\%$

Difficult

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In a chemical reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $B$ was $1.5$ times of $A$ but the equilibrium concentrations of $A$ and $B$ were found to be equal. The equilibrium constant $(K)$ for the aforesaid chemical reaction is

DifficultJEE MAIN 2019

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The amount of $PCl_5$ (in moles) that needs to be added to a $1\,L$ vessel at $250\,^oC$ in order to obtain $0.1\,mol$ of $Cl_2$ for the given reaction is:
$PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$; $K_C = 0.0414\,mol\,L^{-1}$

Medium

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At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.
$(i)$ Find $K_p$.
$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?

Difficult

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$15 \ mol$ of $H_2$ and $5.2 \ mol$ of $I_2$ are mixed and allowed to attain equilibrium at $773 \ K$. At equilibrium,the number of moles of $HI$ is found to be $10$. The equilibrium constant for the dissociation of $HI$ is

MediumAP EAMCET 2024

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For the esterification reaction $CH_3COOH_{(l)} + C_2H_5OH_{(l)} \rightleftharpoons CH_3COOC_2H_{5(l)} + H_2O_{(l)}$,the equilibrium constant $K_c$ is $4$. If $4 \ mol$ of each acid and alcohol are taken initially,what will be the concentration of the acid at equilibrium?

Similar Questions

$AB_{3(g)}$ 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 fraction of $AB_{3(g)}$ is dissociated? .....$\%$

In a chemical reaction $A + 2B \rightleftharpoons 2C + D$,the initial concentration of $B$ was $1.5$ times of $A$ but the equilibrium concentrations of $A$ and $B$ were found to be equal. The equilibrium constant $(K)$ for the aforesaid chemical reaction is

The amount of $PCl_5$ (in moles) that needs to be added to a $1\,L$ vessel at $250\,^oC$ in order to obtain $0.1\,mol$ of $Cl_2$ for the given reaction is:$PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$; $K_C = 0.0414\,mol\,L^{-1}$

At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.$(i)$ Find $K_p$.$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?

$15 \ mol$ of $H_2$ and $5.2 \ mol$ of $I_2$ are mixed and allowed to attain equilibrium at $773 \ K$. At equilibrium,the number of moles of $HI$ is found to be $10$. The equilibrium constant for the dissociation of $HI$ 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 fraction of $AB_{3(g)}$ is dissociated? .....$\%$

The amount of $PCl_5$ (in moles) that needs to be added to a $1\,L$ vessel at $250\,^oC$ in order to obtain $0.1\,mol$ of $Cl_2$ for the given reaction is:
$PCl_5(g) \rightleftharpoons PCl_3(g) + Cl_2(g)$; $K_C = 0.0414\,mol\,L^{-1}$

At $1 \ bar$ pressure and $310 \ K$ temperature,$25\%$ of $N_2O_4$ decomposes. The reaction is: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$.
$(i)$ Find $K_p$.
$(ii)$ At $0.1 \ bar$ pressure and $310 \ K$,what is the percentage of $N_2O_4$ decomposed?