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Question
The decomposition of N2O4 to NO2 was carried out in chloroform at 280°C. At equilibrium, 0.2 mol of N2O4 and 2 × 10−3 mol of NO2 were present in 2 ℓ of the solution. The equilibrium constant for the reaction \[\ce{N2O4 <=> 2NO2}\] is ______.
Options
0.01 × 10−3
2 × 10−3
2 × 10−5
1 × 10−5
MCQ
Fill in the Blanks
Solution
1 × 10−5
Explanation:
| \[\ce{N2O4}\] | \[\ce{<=>}\] | \[\ce{2NO2}\] | |
| At equilibrium | `0.2/2` | `(2 xx 10^-3)/2` | |
| 0.1 | 1 × 10–3 |
Kc = `(["NO"_2]^2)/(["N"_2"O"_4])`
= `(1 xx 10^-3)^2/0.1`
= 1 × 10−5
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Law of Chemical Equilibrium and Equilibrium Constant
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