A sample of O2 gas is collected over water at 23 °C at a barometric pressure of 751 mm Hg (vapour pressure of water at 23°C is 21 mm Hg).The partial pressure of O2 gas in the sample collected is

Question

A sample of O2 gas is collected over water at 23 °C at a barometric pressure of 751 mm Hg (vapour pressure of water at 23°C is 21 mm Hg).The partial pressure of O2 gas in the sample collected is (A) 21 mm Hg (B) 751 mm Hg (C) 0.96 atm (D) 1.02 atm

Tardigrade Admin · Accepted Answer

Using the Dalton's law
P (Total) = Poxygen +Pwater
The vapor pressure of water is

21 mm H g

751 mm H g =

Poxygen

+ 21 mm H g

Poxygen

= 751 mm H g - 21 mm H g

Poxygen

= 730 mm H g

Convert the partial pressure of oxygen in to atmosphere

(730 mm H g) (1 a t m /760 mm H g) = 0.96 a t m

Q. A sample of O2​ gas is collected over water at 23∘C at a barometric pressure of 751mmHg (vapour pressure of water at 23∘C is 21mmHg).The partial pressure of O2​ gas in the sample collected is

21 mm Hg

751 mm Hg

0.96 atm

1.02 atm

Using the Dalton's law P (Total) = Poxygen +Pwater The vapor pressure of water is 21mmHg 751mmHg= Poxygen +21mmHg Poxygen =751mmHg−21mmHg Poxygen =730mmHg Convert the partial pressure of oxygen in to atmosphere (730mmHg)(1atm/760mmHg)=0.96atm

Q. A sample of $O_{2}$ gas is collected over water at $2 3^{\circ} C$ at a barometric pressure of $751 mm H g$ (vapour pressure of water at $2 3^{\circ} C$ is $21 mm H g$ ).The partial pressure of $O_{2}$ gas in the sample collected is

Using the Dalton's law
P (Total) = Poxygen +Pwater
The vapor pressure of water is $21 mm H g$
$751 mm H g =$ Poxygen $+ 21 mm H g$
Poxygen $= 751 mm H g - 21 mm H g$
Poxygen $= 730 mm H g$
Convert the partial pressure of oxygen in to atmosphere
$(730 mm H g) (1 a t m /760 mm H g) = 0.96 a t m$