At 273 , K,which of the following oxides is t | vedclass

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(D) The given reactions represent the decomposition of nitrogen oxides into $N_2$ and $O_2$. Stability is inversely proportional to the equilibrium co

Vedclass · Accepted Answer

$2NO_2 ightleftharpoons N_2 + 2O_2 \, ; \, K_c = 1 	imes 10^{15}$

Vedclass · Answer

(D) The given reactions represent the decomposition of nitrogen oxides into $N_2$ and $O_2$. Stability is inversely proportional to the equilibrium constant $(K_c)$ of the decomposition reaction. $A$ higher $K_c$ value indicates a greater extent of decomposition,meaning the oxide is less stable. $A$ lower $K_c$ value indicates a lesser extent of decomposition,meaning the oxide is more stable. Comparing the given $K_c$ values: $1 	imes 10^{15} Since $2NO_2 ightleftharpoons N_2 + 2O_2$ has the lowest $K_c$ value,$NO_2$ is the most stable among the given options.

At $273 \, K$,which of the following oxides is the most stable?

Similar Questions

For the reaction $2AB \rightleftharpoons A_2 + B_2$,the equilibrium constant is $49$. What will be the equilibrium constant for the reaction $AB \rightleftharpoons 1/2 A_2 + 1/2 B_2$?

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If the equilibrium constants for the given reactions are $K_1$ and $K_2$ respectively,find the relationship between $K_2$ and $K_1$.
$2SO_{2(g)} + O_{2(g)} \rightleftharpoons 2SO_{3(g)}$
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The equilibrium constant $(K_c)$ for the reaction $N_{2(g)} + O_{2(g)} \rightleftharpoons 2 NO_{(g)}$ at temperature $T$ is $4 \times 10^{-4}$. The value of $K_c$ for the reaction $NO_{(g)} \rightleftharpoons \frac{1}{2} N_{2(g)} + \frac{1}{2} O_{2(g)}$ at the same temperature is:

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