Chemistry · Chemical Equilibrium
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1 mole of N2O4 (g) was placed in an empty 1 dm^3 container and allowed to reach equilibrium according to the following equation:
N2O4(g) <-> 2NO2(g)
At equilibrium, x mole Of N2O4 (g) had dissociated. What is the value of the equilibrium constant, Kc, at the temperature of the Experiment?
- A
2x / (1 - x)
- B
4x2 / (1 - x)2
- C
2x / (1 - x)2
- D
4x2 / (1 - x)
This is the following solution:
This expression incorrectly assumes a different relationship between the concentration changes of N2O4 and NO2. It does not account for the stoichiometry of the reaction.
This expression mistakenly squares the denominator, which does not align with the stoichiometry of the equilibrium expression.
This option incorrectly uses an exponent in the denominator, which does not properly reflect the stoichiometry of the reaction.
This is the correct expression. It correctly represents the equilibrium constant Kc for the dissociation of N2O4 into 2NO2, reflecting the stoichiometry of the reaction.
Tagged under Chemistry · Chemical Equilibrium · 2016