1. Tardigrade
  2. Question
  3. Chemistry
  4. 1 mole of NO and 1 mole of O3 are taken in a 10 L vessel and heated. At equilibrium, 50 % of NO (by mass) reacts with O3 according to the equation: NO(g) +O3(g) leftharpoons NO2(g) +O2(g). What will be the equilibrium constant for this reaction?

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Q. $1$ mole of $NO$ and $1$ mole of $O_3$ are taken in a $10\,L$ vessel and heated. At equilibrium, $50\%$ of $NO$ (by mass) reacts with $O_3$ according to the equation:
$NO_{(g)} +O_{3(g)} \rightleftharpoons NO_{2(g)} +O_{2(g)}$.
What will be the equilibrium constant for this reaction?

Equilibrium

Solution:

image
$K_{c}=\frac{0.05\times0.05}{0.05\times0.05}=1$