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Question
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.
Solution
The balanced chemical equation corresponding to the given expression can be written as:
\[\ce{4NO_{(g)} + 6H_2O_{(g)} ↔ 4NH_{3(g)} + 5O_{2(g)}}\]
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RELATED QUESTIONS
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.
- \[\ce{COCl2 (g) ⇌ CO (g) + Cl2 (g)}\]
- \[\ce{CH4 (g) + 2S2 (g) ⇌ CS2 (g) + 2H2S (g)}\]
- \[\ce{CO2 (g) + C (s) ⇌ 2CO (g)}\]
- \[\ce{2H2 (g) + CO (g) ⇌ CH3OH (g)}\]
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- \[\ce{4 NH3 (g) + 5O2 (g) ⇌ 4NO (g) + 6H2O(g)}\]
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 ______.
