Advertisements
Advertisements
प्रश्न
The equilibrium constant expression for a gas reaction is,
`"K"_"c" = (["NH"_3]^4["O"_2]^5)/(["NO"]^4["H"_2"O"]^6)`
Write the balanced chemical equation corresponding to this expression.
उत्तर
The balanced chemical equation corresponding to the given expression can be written as:
\[\ce{4NO_{(g)} + 6H_2O_{(g)} ↔ 4NH_{3(g)} + 5O_{2(g)}}\]
APPEARS IN
संबंधित प्रश्न
Which of the following reactions will get affected by increasing the pressure? Also, mention whether change will cause the reaction to go into forward or backward direction.
- \[\ce{COCl2 (g) ⇌ CO (g) + Cl2 (g)}\]
- \[\ce{CH4 (g) + 2S2 (g) ⇌ CS2 (g) + 2H2S (g)}\]
- \[\ce{CO2 (g) + C (s) ⇌ 2CO (g)}\]
- \[\ce{2H2 (g) + CO (g) ⇌ CH3OH (g)}\]
- \[\ce{CaCO3 (s) ⇌ CaO (s) + CO2 (g)}\]
- \[\ce{4 NH3 (g) + 5O2 (g) ⇌ 4NO (g) + 6H2O(g)}\]
The equilibrium constant for the reaction: \[\ce{N2_{(g)} + O2_{(g)} ⇌ 2NO_{(g)}}\] is 4 × 10–4 at 2000 K. In presence of a catalyst, the equilibrium is attained ten times faster. Therefore, the equilibrium constant in presence of catalyst of 2000 K is ______.
