Assuming that dry air contain $79 % N_{2} a n d 21 % O_{2}$ by volume. Find the density of moist air at $25^{\circ}$ C and 1.0atm when the relative humidity is $60 %$ . The vapour pressure of water at $25^{\circ}$ C is 23.76 mm Hg.

Q. A cylinder contains 0.3 mole

N_{2}

, 0.1 mole

O_{2}

and 0.1 mole

H e

. If the total pressure of gas mixture is 1 atmosphere, the partial pressure of

O_{2}

m m

H g

is:

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Air contains 79% N2 and 21%O2 by volume. If the pressure is 750 mm of Hg, the partial pressure of oxygen (O2) is:

The correct option is A 157.5 mmHgMole Fraction of Oxygen = 0.21Barometric Pressure = 750 mgPartial Pressure of oxygen = Mole Fraction x Barometric PressurePartial Presuure of Oxygen =0.21×750 =157.5 mmHg

Air contains $79 % N_{2}$ and $21 % O_{2}$ by volume. If the pressure is $750 m m$ of $H g$ , the partial pressure of oxygen $(O_{2})$ is:

The correct option is A $157.5 m m H g$
Mole Fraction of Oxygen = 0.21
Barometric Pressure = 750 mg
Partial Pressure of oxygen = Mole Fraction x Barometric Pressure
Partial Presuure of Oxygen $= 0.21 \times 750$
$= 157.5 m m H g$