English, asked by Anonymous, 10 months ago

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 vapour pressure at 27°C is 3.4 kPa. Calculate the number of moles of oxygen collected in the jar.

Answers

Answered by Anonymous
7

Answer:

Given

Volume of oxygen = 50cc=50cm3=50

Atmospheric pressure Po=99.4kPa=99.4Pa

Temperature =27=300.15K

Saturation vapor pressure Ps=3.4kPa=3.4Pa

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=96Pa

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 1.9310-3.

Answered by Anonymous
17

Answer:

Pressure inside the tube

= Atmospheric pressure

= 99.4 K Pa

pressure exerted by O2 vapour

= Atmospheric pressure V.P.

= 99.4 K Pa - 3.4 K Pa

=96 K Pa

Ifνmberofmo≤of O_2=n

Then using gas equation

96×(103)×50×(10−6)

=n×8.3×300

rArr n= ( 96 xx 50 xx (10^3)/8.3 xx 300) =1.9277 xx(10^-3)

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