At constant temperature $200 c m^{3}$ of $N_{2}$ at $720 m m$ and $400 c m^{3}$ of $O_{2}$ at $750 m m$ pressure are put together in a one litre flask.
The final pressure of the mixture is :

111 m m

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222 m m

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333 m m

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444 m m

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Solution

The correct option is C $444 m m$
The number of moles of nitrogen $n = \frac{P V}{R T} = \frac{720 \times 200}{R T}$
The number of moles of oxygen $n^{'} = \frac{P V}{R T} = \frac{750 \times 400}{R T}$

The final pressure $P = \frac{n R T}{V} = \frac{\frac{720 \times 200}{R T} + \frac{750 \times 400}{R T}}{1000} R T = \frac{144000 + 300000}{1000} = 444$ mm.

So, the correct option is $D$

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