Question

The most stable oxide of nitrogen will be:

• A. $2NO\left(g\right)\rightleftharpoons N_2\left(g\right)+O_2\left(g\right);K=2.2\times {10}^{30}$
• B. $2N_{2}O\left(g\right)\rightleftharpoons 2N_2\left(g\right)+O_2\left(g\right);K=3.5\times {10}^{30}$
• C. $2N_2{O}_5\left(g\right)\rightleftharpoons 2N_2\left(g\right)+O_2\left(g\right);K=1.2\times {10}^{24}$
• D. ${NO}_2\left(g\right)\rightleftharpoons 2NO\left(g\right)+O_2\left(g\right);K=6.7\times {10}^{16}$

Answer 1

Answer: (D)

${NO}_2\left(g\right)\rightleftharpoons 2NO\left(g\right)+O_2\left(g\right);K=6.7\times {10}^{16}$

${NO}_2\left(g\right)\rightleftharpoons 2NO\left(g\right)+O_2\left(g\right);K=6.7\times {10}^{16}$
The most stable oxide of nitrogen will be ${NO}_2$ as it has lower value of equilibrium constant.
Stability constant $=\frac{1}{K}$
$\therefore$ Smaller is the value of equilibrium constant greater is the stability of oxide
Other reactions have higher value of equilibrium constant. So these oxides are less stable.