(A) The reaction is $CO + Cl_2 \rightleftharpoons COCl_2$. Initially,$CO = 2\,mol$,$Cl_2 = 3\,mol$,$COCl_2 = 0\,mol$. At equilibrium,$CO = 1\,mol$. Ch

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(A) The reaction is $CO + Cl_2 \rightleftharpoons COCl_2$. Initially,$CO = 2\,mol$,$Cl_2 = 3\,mol$,$COCl_2 = 0\,mol$. At equilibrium,$CO = 1\,mol$. Change in $CO = 2 - 1 = 1\,mol$ reacted. According to stoichiometry,$1\,mol$ of $CO$ reacts with $1\,mol$ of $Cl_2$ to produce $1\,mol$ of $COCl_2$. At equilibrium: $[CO] = \frac{1\,mol}{5\,L} = 0.2\,M$,$[Cl_2] = \frac{3-1\,mol}{5\,L} = \frac{2\,mol}{5\,L} = 0.4\,M$,$[COCl_2] = \frac{1\,mol}{5\,L} = 0.2\,M$. $K_c = \frac{[COCl_2]}{[CO][Cl_2]} = \frac{0.2}{0.2 \times 0.4} = \frac{1}{0.4} = 2.5$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Kp and Kc Relationship

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At a certain temperature in a $5\,L$ vessel,$2\,moles$ of carbon monoxide and $3\,moles$ of chlorine were allowed to reach equilibrium according to the reaction,$CO + Cl_2 \rightleftharpoons COCl_2$. At equilibrium,if $1\,mole$ of $CO$ is present,then the equilibrium constant $(K_c)$ for the reaction is:

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A
$2.5$
B
$4$
C
$2$
D
$3$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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The reaction for which $K_{c} = 2.3 \times 10^3 \ mol \ L^{-1}$ is $-$

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In the thermal dissociation of $PCl_5$,the total pressure in the gaseous equilibrium mixture is $1.0 \ atm$ when half of $PCl_5$ is found to dissociate. The equilibrium constant of the reaction $(K_p)$ in atmosphere is

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$9.2 \ g$ of $N_2O_{4(g)}$ is taken in a closed $1 \ L$ vessel and heated until the following equilibrium is reached: $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$. At equilibrium,$50\%$ of $N_2O_{4(g)}$ is dissociated. What is the equilibrium constant $K_c$ (in $mol \ L^{-1}$)? (Molecular weight of $N_2O_4 = 92$)

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For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$

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One mole of $SO_3$ was placed in a $1 \ L$ reaction vessel at a certain temperature. The following equilibrium was established: $2SO_3 \rightleftharpoons 2SO_2 + O_2$. At equilibrium,$0.6 \ moles$ of $SO_2$ were formed. The equilibrium constant $(K_c)$ of the reaction will be:

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The reaction for which $K_{c} = 2.3 \times 10^3 \ mol \ L^{-1}$ is $-$

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For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$$Z: 2HI \rightleftharpoons H_2 + I_2$

One mole of $SO_3$ was placed in a $1 \ L$ reaction vessel at a certain temperature. The following equilibrium was established: $2SO_3 \rightleftharpoons 2SO_2 + O_2$. At equilibrium,$0.6 \ moles$ of $SO_2$ were formed. The equilibrium constant $(K_c)$ of the reaction will be:

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For the following three equilibria $X, Y$,and $Z$ in the gaseous state at $300 \ K$,the increasing order of the ratio of $K_p$ to $K_c$ is:
$X: 2SO_2 + O_2 \rightleftharpoons 2SO_3$
$Y: PCl_5 \rightleftharpoons PCl_3 + Cl_2$
$Z: 2HI \rightleftharpoons H_2 + I_2$