(B) The given reaction is $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$ with $K_{c1} = 1.8 \times 10^{-6}$.For the target reaction $NO_{(g)} +

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(B) The given reaction is $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$ with $K_{c1} = 1.8 \times 10^{-6}$.For the target reaction $NO_{(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{2(g)}$,we observe that the original reaction is reversed and then multiplied by a factor of $\frac{1}{2}$.Therefore,the new equilibrium constant $K_{c2} = \sqrt{\frac{1}{K_{c1}}}$.$K_{c2} = \sqrt{\frac{1}{1.8 \times 10^{-6}}} = \sqrt{0.555 \times 10^6} = 0.745 \times 10^3 \approx 7.5 \times 10^2$.

Class 11 Chemistry 6-1.Equilibrium (Chemical Equilibrium)Law of equilibrium and Equilibrium constant

Medium

For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $185\,^{\circ}C$. At $185\,^{\circ}C$,the value of $K_c$ for the reaction $NO_{(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{2(g)}$ is

A
$0.9 \times 10^6$
B
$7.5 \times 10^2$
C
$1.95 \times 10^{-3}$
D
$1.95 \times 10^3$

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6-1.Equilibrium (Chemical Equilibrium)

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Law of equilibrium and Equilibrium constant

The value of $K_{c}$ for the reaction $3 O_{2(g)} \longleftrightarrow 2 O_{3(g)}$ is $2.0 \times 10^{-50}$ at $25^{\circ} C$. If the equilibrium concentration of $O_{2}$ in air at $25^{\circ} C$ is $1.6 \times 10^{-2} \, M$,what is the concentration of $O_{3} ?$

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$8 \, \text{mol}$ of $AB_3$ is added to a $1.0 \, \text{dm}^3$ container. If it dissociates according to the reaction $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$ and $2 \, \text{mol}$ of $A_2$ are present at equilibrium,what is the equilibrium constant $(K_c)$ for this reaction?

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For the reactions $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$ and $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$,if the equilibrium constants at $298 \ K$ are $K_1$ and $K_2$ respectively,then the correct relationship between them is .......

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For the formation of $NH_{3(g)}$ from its constituent elements,which of the relations between the reaction quotient $(Q)$ and equilibrium constant $(K_C)$ is correct for the backward reaction?

EasyAP EAMCET 2022

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At $200^{\circ} C$,nitric oxide reacts with oxygen to form nitrogen dioxide as follows: $2 NO(g) + O_2(g) \rightleftharpoons 2 NO_2(g)$,$K_C = 3 \times 10^6$. In a mixture of the three species at equilibrium,we can accurately predict that:

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For the reaction $2NO_{2(g)} \rightleftharpoons 2NO_{(g)} + O_{2(g)}$,$K_c = 1.8 \times 10^{-6}$ at $185\,^{\circ}C$. At $185\,^{\circ}C$,the value of $K_c$ for the reaction $NO_{(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons NO_{2(g)}$ is

Similar Questions

The value of $K_{c}$ for the reaction $3 O_{2(g)} \longleftrightarrow 2 O_{3(g)}$ is $2.0 \times 10^{-50}$ at $25^{\circ} C$. If the equilibrium concentration of $O_{2}$ in air at $25^{\circ} C$ is $1.6 \times 10^{-2} \, M$,what is the concentration of $O_{3} ?$

$8 \, \text{mol}$ of $AB_3$ is added to a $1.0 \, \text{dm}^3$ container. If it dissociates according to the reaction $2AB_{3(g)} \rightleftharpoons A_{2(g)} + 3B_{2(g)}$ and $2 \, \text{mol}$ of $A_2$ are present at equilibrium,what is the equilibrium constant $(K_c)$ for this reaction?

For the reactions $SO_{2(g)} + \frac{1}{2}O_{2(g)} \rightleftharpoons SO_{3(g)}$ and $2SO_{3(g)} \rightleftharpoons 2SO_{2(g)} + O_{2(g)}$,if the equilibrium constants at $298 \ K$ are $K_1$ and $K_2$ respectively,then the correct relationship between them is .......

For the formation of $NH_{3(g)}$ from its constituent elements,which of the relations between the reaction quotient $(Q)$ and equilibrium constant $(K_C)$ is correct for the backward reaction?

At $200^{\circ} C$,nitric oxide reacts with oxygen to form nitrogen dioxide as follows: $2 NO(g) + O_2(g) \rightleftharpoons 2 NO_2(g)$,$K_C = 3 \times 10^6$. In a mixture of the three species at equilibrium,we can accurately predict that:

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