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1mol of Cl(2) and 3 mol of PCl(5) are pl...

`1`mol of `Cl_(2)` and `3` mol of `PCl_(5)` are placed in a `100 L` 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.
`PCl_(5)(g) hArr PCl_(3)(g)+Cl_(2)(g)`

Text Solution

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Total moles of gases at equilibrium = `pV//RT = 2.05 xx 100/(0.082 xx 500)= 5.0`
Out of this 5 moles, 1.0 mole is for and remaining 4 moles
For and its dissociation products.
` PCl_(5) rarr PCl_(3) + Cl_(2)`
`3+x =4 implies x = 1`
Degree of dissociation `= 1/3 = 0.33`
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