Given the reaction: ½ N₂O4(g) --> <-- NO2(g) The equilibrium constant is given as 3.3 at 373K. The value of the equilibrium constant will change if: (1) the partial pressures are given instead of concentrations (2) the temperature is increased to 473K (3) the concentration of the reactant is doubled. 1 and 2 only 1, 2 and 3 2 and 3 only 1 only 2 only M

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Given the reaction: ½ N₂O4(g) --> <--
NO2(g)
The equilibrium constant is given as 3.3
at 373K. The value of the equilibrium constant will change if: (1) the partial pressures
are given instead of concentrations (2) the temperature is increased to 473K (3) the
concentration of the reactant is doubled.
1 and 2 only
1, 2 and 3
2 and 3 only
1 only
2 only
M
Transcribed Image Text:Given the reaction: ½ N₂O4(g) --> <-- NO2(g) The equilibrium constant is given as 3.3 at 373K. The value of the equilibrium constant will change if: (1) the partial pressures are given instead of concentrations (2) the temperature is increased to 473K (3) the concentration of the reactant is doubled. 1 and 2 only 1, 2 and 3 2 and 3 only 1 only 2 only M
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Here this question is asking about equilibrium constant of given reaction.

•Equilibirium constant of a reaction only depends on "TEMPERATURE".

•Equilibirium constant never depend on concentration of reactant and product, pressure of reactant and product, catalyst presence.

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