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PCl(5) (g) to PCl(3) (g) + Cl(2) (g) , D...

`PCl_(5) (g) to PCl_(3) (g) + Cl_(2) (g) , DeltaH^(0) = +124 kJ * mol^(-1)` Applying Le Chatelier's principle , discuss the effect of increase in pressure , temperature and addition of inert gas at constant volume on the equilibrium of this reaction .

Text Solution

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With increase in pressure , the equilibrium will shift towards left i.e., backward reaction will occur to a greater extent . On the other hand with increase in temperature , the equilibrium will shift towards right i.e., forward reaction will occur to a greater extent . With the addition of inert gas at constant volume , the equilibrium will remain undisturbed .
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Knowledge Check

  • Addition of inert gas at constant volume to the equilibrium N_2(g)+3H_2(g)iff2NH_3(g) results.

    A
    Increase in `NH_3` production
    B
    Less production of `NH_3`
    C
    No effect on the reaction
    D
    Increase in magnitude of `K_p`

  • PCl_(5) (g) to PCl_(3) (g) + Cl_(2) (g) , in this chemical reaction -

    A
    `Delta H = Delta E `
    B
    `Delta H gt Delta E`
    C
    `Delta H lt Delta E`
    D
    none of the above