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 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 B $111 m m$
According to the question
Volume of $N_{2} = 200 c m^{3} = 200 m l = 0.2 L$
Pressure of $N_{2}$ =720mm
volume of $O_{2} = 400 c m^{3} = 400 m l = 0.4 L$
pressure of oxygen =750 mm
Total pressure= pressure of nitrogen + pressure of oxygen
$= 720 + 750 = 1470$ mm
As we know volume of flask is 1 liter and pressure is unknown
Using the equation,
$P 1 \times V 1 = P 2 \times V 2$
$1470 \times 0.6 = P 2 \times 1$
$P 2 = 882 m m$ of $H g$ will be the final pressure

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