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NEST2015ChemistryChemical Equilibrium

Consider the following reversible reaction at a particular temperature and pressure, N ₂( ~g )+3 H ₂( ~g ) 2 NH ₃( ~g ) for which the equilibrium constants in terms of mole fraction (x) and partial pressure (p) are defined as K_x= x_ NH ₃ ^2 x_ N ₂ x_ H ₂ ^3 and K_P= p_ NH ₃ ^2 p_ N ₂ p_ H ₂ ^3 , respectively. Let an equilibrium mixture contain 3 mol of N ₂, 1 ~mol of H ₂ and 1 mol of NH ₃ (K_x=8.33 ) . Now, keeping

Options

  1. AThe equilibrium will shift to the left producing more N ₂ , if the N ₂ addition is at constant pressure.
  2. BThe equilibrium will shift to the right producing more NH ₃ , if the N ₂ addition is at constant pressure.
  3. CThe equilibrium will shift to the left producing more N ₂ , if the N ₂ addition is at constant volume.
  4. DThe equilibrium will shift to the right producing more NH ₃ , if the N ₂ addition is at constant volume.

Correct answer

D. The equilibrium will shift to the right producing more NH ₃ , if the N ₂ addition is at constant volume.

Step-by-step solution

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