If a given quantity of PCl5 is heated to 250 degree celsius and allowed to come to equilibrium at atmospheric pressure it is found to be dissociated to the extent of 80% into PCl3 and chlorine. If now, the pressure on this mixture is increased so that finally the equilibrium mixture occupies only one half of its original volume ( temperature maintained constant).i) What will the % dissociation at the new pressure?ii) What will be the effect of adding He gas keeping the volume fixed at V/2?

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Q. At a given temperature the following reaction is allowed to reach equilibrium in a vessel of volume

V_{1}

litre. The degree of dissociation is

α_{1}

. If by keeping the temperature fixed the volume of the reaction vessel is doubled (assuming the degrees of dissociation to be small) the new degree of dissociation shall be :

P C l_{5} ⇌ P C l_{3} + C l_{2}

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27^{0} C

a gas is compressed to half of its volume.To what temperature it must now be heated at constant pressure so that gas occupies just its original volume?

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dissociates as

P C l_{5} (g) ⇌ P C l_{3} (g) + C l_{2} (g) .

If total pressure at equilibrium of the reaction mixture is P and degree of dissociation of

P C l_{5}

is x, the partial pressure of

P C l_{3}

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