229228 If the equilibrium constant for the reaction $2 \mathrm{AB} \rightleftharpoons A_{2}+B_{2}$ is 49.What is the value of equilibrium constant for
$\mathbf{A B} \rightleftharpoons \frac{\mathbf{1}}{\mathbf{2}} \mathbf{A}_{2}+\frac{\mathbf{1}}{\mathbf{2}} \mathbf{B}_{2} \text { ? }$

229293 For equilibrium $\mathbf{P C l}_{5}(\mathbf{g})$ $K_{p}$ and $K_{c}$ will hold the following relationship

229229 $\mathrm{A}(\mathrm{g})+3 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \quad 4 \mathrm{C}(\mathrm{g})$ is a reversible reaction where all the reactants and product are in gaseous state.
Conditions:
(i) Concentrations of both $A$ and $B$ are equal at the initiation
(ii) Concentration of both $\mathrm{A}$ and $\mathrm{C}$ are equal at the equilibrium.
Considering the imposed condition, find the value of $K_{c}$ of this reversible reaction.

229230 The reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{SO}_{3}(\mathrm{~g})$ was carried out in a closed vessel of $1 \mathrm{~L}$ capacity at a suitable temperature. The initial concentrations of $\mathrm{SO}_{2}$ and $\mathrm{O}_{2}$ are 2 and 1 moles/L respectively. At equilibrium, 1.6 moles of $\mathrm{SO}_{3}(\mathrm{~g})$ was found. The value of $\mathrm{K}_{\mathrm{c}}$ at the same temperature is

229231 Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $\mathbf{2 A}_{(\mathrm{g})} \rightleftharpoons \quad \mathbf{B}_{(\mathrm{g})}+\mathbf{C}_{(\mathrm{g})}$

229228 If the equilibrium constant for the reaction $2 \mathrm{AB} \rightleftharpoons A_{2}+B_{2}$ is 49.What is the value of equilibrium constant for
$\mathbf{A B} \rightleftharpoons \frac{\mathbf{1}}{\mathbf{2}} \mathbf{A}_{2}+\frac{\mathbf{1}}{\mathbf{2}} \mathbf{B}_{2} \text { ? }$

229293 For equilibrium $\mathbf{P C l}_{5}(\mathbf{g})$ $K_{p}$ and $K_{c}$ will hold the following relationship

229229 $\mathrm{A}(\mathrm{g})+3 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \quad 4 \mathrm{C}(\mathrm{g})$ is a reversible reaction where all the reactants and product are in gaseous state.
Conditions:
(i) Concentrations of both $A$ and $B$ are equal at the initiation
(ii) Concentration of both $\mathrm{A}$ and $\mathrm{C}$ are equal at the equilibrium.
Considering the imposed condition, find the value of $K_{c}$ of this reversible reaction.

229230 The reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{SO}_{3}(\mathrm{~g})$ was carried out in a closed vessel of $1 \mathrm{~L}$ capacity at a suitable temperature. The initial concentrations of $\mathrm{SO}_{2}$ and $\mathrm{O}_{2}$ are 2 and 1 moles/L respectively. At equilibrium, 1.6 moles of $\mathrm{SO}_{3}(\mathrm{~g})$ was found. The value of $\mathrm{K}_{\mathrm{c}}$ at the same temperature is

229231 Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $\mathbf{2 A}_{(\mathrm{g})} \rightleftharpoons \quad \mathbf{B}_{(\mathrm{g})}+\mathbf{C}_{(\mathrm{g})}$

229228 If the equilibrium constant for the reaction $2 \mathrm{AB} \rightleftharpoons A_{2}+B_{2}$ is 49.What is the value of equilibrium constant for
$\mathbf{A B} \rightleftharpoons \frac{\mathbf{1}}{\mathbf{2}} \mathbf{A}_{2}+\frac{\mathbf{1}}{\mathbf{2}} \mathbf{B}_{2} \text { ? }$

229293 For equilibrium $\mathbf{P C l}_{5}(\mathbf{g})$ $K_{p}$ and $K_{c}$ will hold the following relationship

229229 $\mathrm{A}(\mathrm{g})+3 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \quad 4 \mathrm{C}(\mathrm{g})$ is a reversible reaction where all the reactants and product are in gaseous state.
Conditions:
(i) Concentrations of both $A$ and $B$ are equal at the initiation
(ii) Concentration of both $\mathrm{A}$ and $\mathrm{C}$ are equal at the equilibrium.
Considering the imposed condition, find the value of $K_{c}$ of this reversible reaction.

229230 The reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{SO}_{3}(\mathrm{~g})$ was carried out in a closed vessel of $1 \mathrm{~L}$ capacity at a suitable temperature. The initial concentrations of $\mathrm{SO}_{2}$ and $\mathrm{O}_{2}$ are 2 and 1 moles/L respectively. At equilibrium, 1.6 moles of $\mathrm{SO}_{3}(\mathrm{~g})$ was found. The value of $\mathrm{K}_{\mathrm{c}}$ at the same temperature is

229231 Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $\mathbf{2 A}_{(\mathrm{g})} \rightleftharpoons \quad \mathbf{B}_{(\mathrm{g})}+\mathbf{C}_{(\mathrm{g})}$

229228 If the equilibrium constant for the reaction $2 \mathrm{AB} \rightleftharpoons A_{2}+B_{2}$ is 49.What is the value of equilibrium constant for
$\mathbf{A B} \rightleftharpoons \frac{\mathbf{1}}{\mathbf{2}} \mathbf{A}_{2}+\frac{\mathbf{1}}{\mathbf{2}} \mathbf{B}_{2} \text { ? }$

229293 For equilibrium $\mathbf{P C l}_{5}(\mathbf{g})$ $K_{p}$ and $K_{c}$ will hold the following relationship

229229 $\mathrm{A}(\mathrm{g})+3 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \quad 4 \mathrm{C}(\mathrm{g})$ is a reversible reaction where all the reactants and product are in gaseous state.
Conditions:
(i) Concentrations of both $A$ and $B$ are equal at the initiation
(ii) Concentration of both $\mathrm{A}$ and $\mathrm{C}$ are equal at the equilibrium.
Considering the imposed condition, find the value of $K_{c}$ of this reversible reaction.

229230 The reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{SO}_{3}(\mathrm{~g})$ was carried out in a closed vessel of $1 \mathrm{~L}$ capacity at a suitable temperature. The initial concentrations of $\mathrm{SO}_{2}$ and $\mathrm{O}_{2}$ are 2 and 1 moles/L respectively. At equilibrium, 1.6 moles of $\mathrm{SO}_{3}(\mathrm{~g})$ was found. The value of $\mathrm{K}_{\mathrm{c}}$ at the same temperature is

229231 Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $\mathbf{2 A}_{(\mathrm{g})} \rightleftharpoons \quad \mathbf{B}_{(\mathrm{g})}+\mathbf{C}_{(\mathrm{g})}$

229228 If the equilibrium constant for the reaction $2 \mathrm{AB} \rightleftharpoons A_{2}+B_{2}$ is 49.What is the value of equilibrium constant for
$\mathbf{A B} \rightleftharpoons \frac{\mathbf{1}}{\mathbf{2}} \mathbf{A}_{2}+\frac{\mathbf{1}}{\mathbf{2}} \mathbf{B}_{2} \text { ? }$

229293 For equilibrium $\mathbf{P C l}_{5}(\mathbf{g})$ $K_{p}$ and $K_{c}$ will hold the following relationship

229229 $\mathrm{A}(\mathrm{g})+3 \mathrm{~B}(\mathrm{~g}) \rightleftharpoons \quad 4 \mathrm{C}(\mathrm{g})$ is a reversible reaction where all the reactants and product are in gaseous state.
Conditions:
(i) Concentrations of both $A$ and $B$ are equal at the initiation
(ii) Concentration of both $\mathrm{A}$ and $\mathrm{C}$ are equal at the equilibrium.
Considering the imposed condition, find the value of $K_{c}$ of this reversible reaction.

229230 The reaction $2 \mathrm{SO}_{2}(\mathrm{~g})+\mathrm{O}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{SO}_{3}(\mathrm{~g})$ was carried out in a closed vessel of $1 \mathrm{~L}$ capacity at a suitable temperature. The initial concentrations of $\mathrm{SO}_{2}$ and $\mathrm{O}_{2}$ are 2 and 1 moles/L respectively. At equilibrium, 1.6 moles of $\mathrm{SO}_{3}(\mathrm{~g})$ was found. The value of $\mathrm{K}_{\mathrm{c}}$ at the same temperature is

229231 Which among the following denotes the correct relationship between $K_{p}$ and $K_{c}$ for the reaction $\mathbf{2 A}_{(\mathrm{g})} \rightleftharpoons \quad \mathbf{B}_{(\mathrm{g})}+\mathbf{C}_{(\mathrm{g})}$