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At 27^(@)C NO and Cl(2) gases are introd...

At `27^(@)C` NO and `Cl_(2)` gases are introduced in a 10 litre flask such that their initial partial pressures are 20 and 16 atm respectively. The flask already contains 24 g of magnesium. After some time, the amount of magnesium left was 0.2 moles due to the establishment of following two equilibria
`2NO(g)+Cl_(2)(g) hArr 2NOCl(g)`
`Mg(s)+Cl_(2)(g) hArr 2MgCl_(2)(s), K_(p)=0.2 "atm"^(-1)`
The final pressure of NOCl would be

A

7.84 atm

B

18.06 atm

C

129.6 atm

D

64.8 atm

Text Solution

Verified by Experts

The correct Answer is:
B
`K_(p)=0.2=(1)/(P_(Cl_(2))) rArr P_(Cl_(2))` at equilibrium = 5 atm
`2NO(g)+Cl_(2)(g) hArr 2NOCl(g) `
`{:("Initially",20,16,0),("At equi.", 20-2x,16-x-y, 2x):}`

`Cl_(2)(g)+Mg(s) hArr 2MgCl_(2)(s)`
`{:("Initially",16,1,0),("At equi.", 16-x-y,1-z,),(,,=0.2,):}`
`z=0.8` moles of Mg that react with 0.8 moles of `Cl_(2)` (Since z is the moles while y is pressure in atm)
`y=(0.8xx0.082xx300)/(10)=1.97` atm
We know that,
`16-x-y=5`
or, `x=9.03, P_(NOCl)=18.06` atm
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