Medium
The least stable oxide of nitrogen is:
- A$2NO_{2(g)} \rightleftharpoons N_{2(g)} + 2O_{2(g)}; K_{eq} = 6.7 \times 10^{16} \ mol \ L^{-1}$
- B$2N_2O_{5(g)} \rightleftharpoons 2N_{2(g)} + 5O_{2(g)}; K_{eq} = 1.2 \times 10^{24} \ mol^5 \ L^{-5}$
- C$2NO_{(g)} \rightleftharpoons N_{2(g)} + O_{2(g)}; K_{eq} = 2.2 \times 10^{30}$
- D$2N_2O_{(g)} \rightleftharpoons 2N_{2(g)} + O_{2(g)}; K_{eq} = 3.5 \times 10^{33} \ mol \ L^{-1}$
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Similar Questions
If the equilibrium constant for $2 SO_2 + O_2 \rightleftharpoons 2 SO_3$ is $K$,then the equilibrium constant for $SO_3 \rightleftharpoons SO_2 + \frac{1}{2} O_2$ will be :
Medium
View SolutionFor the system $3A + 2B \rightleftharpoons C$,the expression for equilibrium constant is
Medium
View SolutionThe following concentrations were observed at $500 \ K$ for the formation of $NH_3$ from $N_2$ and $H_2$. At equilibrium: $[N_2] = 2 \times 10^{-2} \ M$,$[H_2] = 3 \times 10^{-2} \ M$ and $[NH_3] = 1.5 \times 10^{-2} \ M$. The equilibrium constant for the reaction is:
DifficultJEE MAIN 2024
View SolutionConsider the following reactions in which all the reactants and products are present in gaseous state:
$2xy \rightleftharpoons x_2 + y_2$ $K_1 = 2.5 \times 10^5$
$xy + \frac{1}{2}z_2 \rightleftharpoons xyz$ $K_2 = 5 \times 10^{-3}$
The value of $K_3$ for the equilibrium $\frac{1}{2}x_2 + \frac{1}{2}y_2 + \frac{1}{2}z_2 \rightleftharpoons xyz$ is:
$2xy \rightleftharpoons x_2 + y_2$ $K_1 = 2.5 \times 10^5$
$xy + \frac{1}{2}z_2 \rightleftharpoons xyz$ $K_2 = 5 \times 10^{-3}$
The value of $K_3$ for the equilibrium $\frac{1}{2}x_2 + \frac{1}{2}y_2 + \frac{1}{2}z_2 \rightleftharpoons xyz$ is:
DifficultJEE MAIN 2026
View SolutionAt $200^{\circ} C$,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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