$P \to Q$ , the half life of the reaction was 3 hour, when the initial concentration of P was $0.5 M$ . As the concentation of P was increased to $1 M$ , half life changes to 6 hours. The order of reaction with respect to P is:

Q. For the reaction:

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

At constant pressure, the presence of inert gases:

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For the reaction : P⇌Q+R. Initially 2 mol of P was taken. Up to equailibrium 0.5mol of P was dissociated. What would be the degree of dissociation;-

The correct option is B 0.5P⇀↽ Q+RInitially 2 moles 0 0At equilibrium 2-0.5 0.5 0.5α=no.ofmolesdissociatedintoionstotalmolesinitiallytaken=0.5+0.52=12 =0.5Therefore α =0.5

For the reaction : $P ⇌ Q + R$ . Initially 2 mol of $P$ was taken. Up to equailibrium $0.5 m o l$ of $P$ was dissociated. What would be the degree of dissociation;-

The correct option is B $0.5$
P $_{↽}^{⇀}$ Q+R
Initially 2 moles 0 0
At equilibrium 2-0.5 0.5 0.5
$α = \frac{n o . o f m o l e s d i s s o c i a t e d i n t o i o n s}{t o t a l m o l e s i n i t i a l l y t a k e n} = \frac{0.5 + 0.5}{2} = \frac{1}{2}$ =0.5
Therefore $α$ =0.5