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Question
For the reaction,
\[\ce{N2 + O2(g) ⇌ 2NO(g)}\]
the equilibrium constant is K1. The equilibrium constant is K2 for the reaction
\[\ce{2NO(g) + O2(g) ⇌ 2NO2(g)}\]
What is "K" for the reaction:
\[\ce{NO2(g) ⇌ 1/2 N2(g) + O2(g)}\]?
Options
`1/(("K"_1"K"_2))`
`1/((2"K"_1"K"_2))`
`1/((4"K"_1"K"_2))`
`[1/(("K"_1"K"_2))]^(1/2)`
MCQ
Solution
`[1/(("K"_1"K"_2))]^(1/2)`
Explanation:
\[\ce{N2(g) + O2(g) ⇌ 2NO(g)}\], K1
\[\ce{2NO(g) + O2(g) ⇌ 2NO2(g)}\], K2
\[\ce{N2(g) + 2O2(g) ⇌ 2NO2(g)}\], K = K1 × K2
∴ for \[\ce{NO2(g) ⇌ 1/2 N2(g) + O2(g)}\]
K = `[1/(("K"_1"K"_2))]^(1/2)`
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Law of Chemical Equilibrium and Equilibrium Constant
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