Q. 565.0( 1 Vote )

# 50 cc of oxygen is collected in an inverted gas jar over water. The atmospheric pressure is 99.4 kPa and the room temperature is 27°C. The water level in the jar is same as the level outside. The saturation vapor pressure at 27°C is 3.4 kPa. Calculate the number of moles of oxygen collected in the jar.

Given

Volume of oxygen = 50cc=50cm3=50 Atmospheric pressure Po=99.4kPa=99.4 Pa

Temperature =27 =300.15K

Saturation vapor pressure Ps=3.4kPa=3.4 Pa

According to question water level in the jar is same as level outside. So

Pressure inside the jar = pressure outside the jar

Pressure outside the jar =atmospheric pressure Po

Pressure inside the jar=Po …. (1)

But

Pressure inside the jar is also = vapor pressure of oxygen+ Saturation vapor pressure

Pressure inside the jar=P+Ps …. (2)

From equation (1) and (2), we can write

Po=P+Ps

P=Po-Ps=99.4 -3.4 =96 Pa

Applying ideal gas equation

PV=nRT

Where V= volume of gas

R=gas constant =8.3JK-1mol-1

T=temperature

n=number of moles of gas

P=pressure of gas.   The number of moles of oxygen collected in the jar is 1.93 10-3.

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