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JEE Main20205 Sep 2020Morning ShiftChemistryChemical EquilibriumActual

Consider the following reaction: N 2 O 4 ( g ) = 2 NO 2 ( g ) :   Δ H 0 = + 58 k For each of the following cases ( a ,   b ) , the direction in which the equilibrium shifts is: (a) Temperature is decreased. (b) Pressure is increased by adding N 2 at constant T.

Options

  1. A(a) towards product, (b) towards reactant
  2. B(a) towards reactant, (b) towards product
  3. C(a) towards reactant, (b) no change
  4. D(a) towards product, (b) no change

Correct answer

C. (a) towards reactant, (b) no change

Step-by-step solution

(i) As reaction is endothermic so on decrease in temperature equilibrium shift in reactant side. (ii) On increase in pressure by adding inert gas at same temperature, no shifting will take place

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