1 mole of nitrogen and 3 moles of $$PCl_5$$ are placed in 100lit vessel heated to $$227^C$$. The equilibrium pressure is 2.05 atm. Assuming ideal behaviour, calculate the degree of dissociation for $$PCl_5$$ and $$K_P$$ for the reaction,

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Q8.one mole of N2 and 3 moles of PCl5 are placed in a 100l vessel heated to 227C the equilibrium pressure is 2.05 atm assuming ideal behaviour calculate the degree of dissociation for PCl5 and kp for the reaction PCl5--> PCl3 +Cl2

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One mole of

N_{2}

and

3 m o l e s

P C l_{5}

are placed in a

100

litre vessel heated to

227^{\circ} C

. The equilibrium pressure is

2.05

atm. Assuming ideal behaviour, calculate degree of dissociation of

P C l_{5}

and

K_{p}

of the reaction:

P C l_{5} ⇌ P C l_{3} + C l_{2}

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1.0 m o l e

of nitrogen and

3.0 m o l e s

P {C l}_{5}

are placed in

100 L

vessel heated to

227^{o} C

. The equilibrium pressure is

2.05 a t m

. Assuming ideal behaviour, calculate the degree of dissociation for

P {C l}_{5}

and

K_{p}

for the reaction,

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

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One mole of $N_{2} a n d 3$ moles of $P C l_{5}$ are placed in a 100 litre vessel heated to $227^{\circ} C$ . The equilibrium pressure is 2.05 atm. Assuming ideal behaviour, calculate degree of dissociation of $P C l_{5}$ for the reaction $P C l_{5} ⇌ P C l_{3} + C l_{2}$ .

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At $227^{o} C$ one mole of $C l_{2}$ and 3 moles of $P C l_{5}$ are placed in a 100 litre container and allowed to reach equilibrium. It is found that the equilibrium pressure is 2.05 atmospheres. Assuming ideal behaviour, the degree of dissociation 'x' for $P C l_{5}$ and $K_{p}$ for the reaction $P C l_{5}$ (g) $⇌$ $P C l_{3}$ (g) + $C l_{2}$ (g) is:

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