229237 At a certain temperature, 2 mole of $\mathrm{CO}$ and 4 moles of $\mathrm{Cl}_{2}$ gases were reacted to form $\mathrm{COCl}_{2}$ in a $10 \mathrm{~L}$ vessel. At equilibrium if one mole of $\mathrm{CO}$ is present then equilibrium constant for the reaction is

229238 Two solids dissociate as follows: $\mathbf{A}(\mathbf{s}) \rightleftharpoons \mathbf{B}(\mathbf{g})+\mathbf{C}(\mathbf{g}) ; \mathbf{K}_{\mathrm{p}_{1}}=\mathbf{x} \mathbf{a t m}^{2}$
$\mathrm{D}(\mathrm{s}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{E}(\mathrm{g}) ; \mathrm{K}_{\mathrm{p}_{2}}=\mathrm{y} \mathbf{a t m}^{2}$ The total pressure when both the solids dissociate simultaneously is

229239 $2 \mathrm{ICl} \rightarrow \mathrm{I}_{2}+\mathrm{Cl}_{2} ; \mathrm{K}_{\mathrm{c}}=0.14$
If initial concentration of $\mathrm{ICl}$ is $0.6 \mathrm{M}$, then equilibrium concentration of $I_{2}$ is:

229240 What will be the equilibrium constant of the given reaction carried out in a $5 \mathrm{~L}$ vessel and having equilibrium amounts of $A_{2}$ and $A$ as 0.5 mole and $2 \times 10^{-6}$ mole respectively?
The reaction: $A_{2} \rightleftharpoons 2 \mathrm{~A}$

229237 At a certain temperature, 2 mole of $\mathrm{CO}$ and 4 moles of $\mathrm{Cl}_{2}$ gases were reacted to form $\mathrm{COCl}_{2}$ in a $10 \mathrm{~L}$ vessel. At equilibrium if one mole of $\mathrm{CO}$ is present then equilibrium constant for the reaction is

229238 Two solids dissociate as follows: $\mathbf{A}(\mathbf{s}) \rightleftharpoons \mathbf{B}(\mathbf{g})+\mathbf{C}(\mathbf{g}) ; \mathbf{K}_{\mathrm{p}_{1}}=\mathbf{x} \mathbf{a t m}^{2}$
$\mathrm{D}(\mathrm{s}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{E}(\mathrm{g}) ; \mathrm{K}_{\mathrm{p}_{2}}=\mathrm{y} \mathbf{a t m}^{2}$ The total pressure when both the solids dissociate simultaneously is

229239 $2 \mathrm{ICl} \rightarrow \mathrm{I}_{2}+\mathrm{Cl}_{2} ; \mathrm{K}_{\mathrm{c}}=0.14$
If initial concentration of $\mathrm{ICl}$ is $0.6 \mathrm{M}$, then equilibrium concentration of $I_{2}$ is:

229240 What will be the equilibrium constant of the given reaction carried out in a $5 \mathrm{~L}$ vessel and having equilibrium amounts of $A_{2}$ and $A$ as 0.5 mole and $2 \times 10^{-6}$ mole respectively?
The reaction: $A_{2} \rightleftharpoons 2 \mathrm{~A}$

229237 At a certain temperature, 2 mole of $\mathrm{CO}$ and 4 moles of $\mathrm{Cl}_{2}$ gases were reacted to form $\mathrm{COCl}_{2}$ in a $10 \mathrm{~L}$ vessel. At equilibrium if one mole of $\mathrm{CO}$ is present then equilibrium constant for the reaction is

229238 Two solids dissociate as follows: $\mathbf{A}(\mathbf{s}) \rightleftharpoons \mathbf{B}(\mathbf{g})+\mathbf{C}(\mathbf{g}) ; \mathbf{K}_{\mathrm{p}_{1}}=\mathbf{x} \mathbf{a t m}^{2}$
$\mathrm{D}(\mathrm{s}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{E}(\mathrm{g}) ; \mathrm{K}_{\mathrm{p}_{2}}=\mathrm{y} \mathbf{a t m}^{2}$ The total pressure when both the solids dissociate simultaneously is

229239 $2 \mathrm{ICl} \rightarrow \mathrm{I}_{2}+\mathrm{Cl}_{2} ; \mathrm{K}_{\mathrm{c}}=0.14$
If initial concentration of $\mathrm{ICl}$ is $0.6 \mathrm{M}$, then equilibrium concentration of $I_{2}$ is:

229240 What will be the equilibrium constant of the given reaction carried out in a $5 \mathrm{~L}$ vessel and having equilibrium amounts of $A_{2}$ and $A$ as 0.5 mole and $2 \times 10^{-6}$ mole respectively?
The reaction: $A_{2} \rightleftharpoons 2 \mathrm{~A}$

229237 At a certain temperature, 2 mole of $\mathrm{CO}$ and 4 moles of $\mathrm{Cl}_{2}$ gases were reacted to form $\mathrm{COCl}_{2}$ in a $10 \mathrm{~L}$ vessel. At equilibrium if one mole of $\mathrm{CO}$ is present then equilibrium constant for the reaction is

229238 Two solids dissociate as follows: $\mathbf{A}(\mathbf{s}) \rightleftharpoons \mathbf{B}(\mathbf{g})+\mathbf{C}(\mathbf{g}) ; \mathbf{K}_{\mathrm{p}_{1}}=\mathbf{x} \mathbf{a t m}^{2}$
$\mathrm{D}(\mathrm{s}) \rightleftharpoons \mathrm{C}(\mathrm{g})+\mathrm{E}(\mathrm{g}) ; \mathrm{K}_{\mathrm{p}_{2}}=\mathrm{y} \mathbf{a t m}^{2}$ The total pressure when both the solids dissociate simultaneously is

229239 $2 \mathrm{ICl} \rightarrow \mathrm{I}_{2}+\mathrm{Cl}_{2} ; \mathrm{K}_{\mathrm{c}}=0.14$
If initial concentration of $\mathrm{ICl}$ is $0.6 \mathrm{M}$, then equilibrium concentration of $I_{2}$ is:

229240 What will be the equilibrium constant of the given reaction carried out in a $5 \mathrm{~L}$ vessel and having equilibrium amounts of $A_{2}$ and $A$ as 0.5 mole and $2 \times 10^{-6}$ mole respectively?
The reaction: $A_{2} \rightleftharpoons 2 \mathrm{~A}$