228945 At a certain temperature, equilibrium constant $\left(K_{c}\right)$ is 16 for the reaction.
$\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \text \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{NO}(\mathrm{g})$
If one mole of each of the four gases are taken in one litre container, the equilibrium concentration of $\mathrm{NO}$ will be

228946 The equilibrium constant for the reaction, $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NH}_{3}(\mathrm{~g})$ and, $2 \mathrm{~N}_{2}(\mathrm{~g})+\mathbf{6 H _ { 2 }}$ $\rightleftharpoons \quad 4 \mathrm{NH}_{3}(\mathrm{~g})$ are $K_{1}$ and $K_{2}$, respectively. The relationship between $K_{1}$ and $K_{2}$ is

228948 Change in volume of the system does not alter the number of moles in which of the following equilibrium ?

228949 For $2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}$, rate and rate constants are $2 \times 10^{-3}$ and $4 \times 10^{-4}$ respectively. Then the concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ at that time will be

228945 At a certain temperature, equilibrium constant $\left(K_{c}\right)$ is 16 for the reaction.
$\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \text \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{NO}(\mathrm{g})$
If one mole of each of the four gases are taken in one litre container, the equilibrium concentration of $\mathrm{NO}$ will be

228946 The equilibrium constant for the reaction, $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NH}_{3}(\mathrm{~g})$ and, $2 \mathrm{~N}_{2}(\mathrm{~g})+\mathbf{6 H _ { 2 }}$ $\rightleftharpoons \quad 4 \mathrm{NH}_{3}(\mathrm{~g})$ are $K_{1}$ and $K_{2}$, respectively. The relationship between $K_{1}$ and $K_{2}$ is

228948 Change in volume of the system does not alter the number of moles in which of the following equilibrium ?

228949 For $2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}$, rate and rate constants are $2 \times 10^{-3}$ and $4 \times 10^{-4}$ respectively. Then the concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ at that time will be

228945 At a certain temperature, equilibrium constant $\left(K_{c}\right)$ is 16 for the reaction.
$\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \text \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{NO}(\mathrm{g})$
If one mole of each of the four gases are taken in one litre container, the equilibrium concentration of $\mathrm{NO}$ will be

228946 The equilibrium constant for the reaction, $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NH}_{3}(\mathrm{~g})$ and, $2 \mathrm{~N}_{2}(\mathrm{~g})+\mathbf{6 H _ { 2 }}$ $\rightleftharpoons \quad 4 \mathrm{NH}_{3}(\mathrm{~g})$ are $K_{1}$ and $K_{2}$, respectively. The relationship between $K_{1}$ and $K_{2}$ is

228948 Change in volume of the system does not alter the number of moles in which of the following equilibrium ?

228949 For $2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}$, rate and rate constants are $2 \times 10^{-3}$ and $4 \times 10^{-4}$ respectively. Then the concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ at that time will be

228945 At a certain temperature, equilibrium constant $\left(K_{c}\right)$ is 16 for the reaction.
$\mathrm{SO}_{2}(\mathrm{~g})+\mathrm{NO}_{2}(\mathrm{~g}) \text \mathrm{SO}_{3}(\mathrm{~g})+\mathrm{NO}(\mathrm{g})$
If one mole of each of the four gases are taken in one litre container, the equilibrium concentration of $\mathrm{NO}$ will be

228946 The equilibrium constant for the reaction, $\mathrm{N}_{2}(\mathrm{~g})+3 \mathrm{H}_{2}(\mathrm{~g}) \rightleftharpoons \quad 2 \mathrm{NH}_{3}(\mathrm{~g})$ and, $2 \mathrm{~N}_{2}(\mathrm{~g})+\mathbf{6 H _ { 2 }}$ $\rightleftharpoons \quad 4 \mathrm{NH}_{3}(\mathrm{~g})$ are $K_{1}$ and $K_{2}$, respectively. The relationship between $K_{1}$ and $K_{2}$ is

228948 Change in volume of the system does not alter the number of moles in which of the following equilibrium ?

228949 For $2 \mathrm{~N}_{2} \mathrm{O}_{5} \rightarrow 4 \mathrm{NO}_{2}+\mathrm{O}_{2}$, rate and rate constants are $2 \times 10^{-3}$ and $4 \times 10^{-4}$ respectively. Then the concentration of $\mathrm{N}_{2} \mathrm{O}_{5}$ at that time will be