(D) The equilibrium constant $K_c$ depends on the units of concentration if the change in the number of moles of gaseous species,$\Delta n_g$,is non-z

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$COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$

(D) The equilibrium constant $K_c$ depends on the units of concentration if the change in the number of moles of gaseous species,$\Delta n_g$,is non-zero.For option $A$: $\Delta n_g = (0.5 + 0.5) - 1 = 0$.For option $B$: $\Delta n_g = 0$ (as only aqueous species are involved in the expression).For option $C$: $\Delta n_g = 0$ (as liquid species are not included in the $K_c$ expression).For option $D$: $\Delta n_g = (1 + 1) - 1 = 1$.Since $\Delta n_g \neq 0$ for reaction $D$,the equilibrium constant $K_c$ depends on the units of concentration.

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

Medium

For which of the following reactions does the equilibrium constant depend on the units of concentration?

AIIMS 1983 All AIIMS

A
$NO_{(g)} \rightleftharpoons \frac{1}{2}N_{2(g)} + \frac{1}{2}O_{2(g)}$
B
$Zn_{(s)} + Cu^{2+}_{(aq)} \rightleftharpoons Cu_{(s)} + Zn^{2+}_{(aq)}$
C
$C_2H_5OH_{(l)} + CH_3COOH_{(l)} \rightleftharpoons CH_3COOC_2H_{5(l)} + H_2O_{(l)}$ (Reaction carried in an inert solvent)
D
$COCl_{2(g)} \rightleftharpoons CO_{(g)} + Cl_{2(g)}$

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6-1.Equilibrium (Chemical Equilibrium)

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Kp and Kc Relationship

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AIIMS 1983 Paper All AIIMS years →

For the reaction $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,if $P_{Br_2} = \frac{P}{9}$ at equilibrium and $P$ is the total pressure,find the value of $\frac{K_P}{P}$.

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$9.2 \ g$ of $N_2O_{4(g)}$ is taken in a $1 \ L$ closed vessel and heated until the following equilibrium is attained:
${N_2}{O_{4(g)}} \rightleftharpoons 2N{O_{2(g)}}$
If $50\%$ of $N_2O_{4(g)}$ dissociates at equilibrium,what will be the equilibrium constant (in $mol \ L^{-1}$)? (Mol. wt. of $N_2O_4 = 92$)

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In a $500 \,mL$ flask,the degree of dissociation of $PCl_5$ at equilibrium is $40 \%$ and the initial amount is $5 \,moles$. The value of equilibrium constant in $mol \,L^{-1}$ for the decomposition of $PCl_5$ is

DifficultAP EAMCET 2008

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For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Given $R = 0.0831 \, kJ/(mol \cdot K)$,when $K_p$ and $K_c$ are compared at $184 \, ^\circ C$,it is found that:

MediumAIEEE 2005

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For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,the observed total pressure of the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^\circ C$. The value of $K_P$ for the reaction is: (in $atm^2$)

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For which of the following reactions does the equilibrium constant depend on the units of concentration?

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For the reaction $2NOBr_{(g)} \rightleftharpoons 2NO_{(g)} + Br_{2(g)}$,if $P_{Br_2} = \frac{P}{9}$ at equilibrium and $P$ is the total pressure,find the value of $\frac{K_P}{P}$.

In a $500 \,mL$ flask,the degree of dissociation of $PCl_5$ at equilibrium is $40 \%$ and the initial amount is $5 \,moles$. The value of equilibrium constant in $mol \,L^{-1}$ for the decomposition of $PCl_5$ is

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $184 \, ^\circ C$. Given $R = 0.0831 \, kJ/(mol \cdot K)$,when $K_p$ and $K_c$ are compared at $184 \, ^\circ C$,it is found that:

For the reaction $NH_4HS_{(s)} \rightleftharpoons NH_{3(g)} + H_2S_{(g)}$,the observed total pressure of the reaction mixture at equilibrium is $1.12 \ atm$ at $106 \ ^\circ C$. The value of $K_P$ for the reaction is: (in $atm^2$)

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