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Chapter 12: Q12.118CP (page 497)

In an experiment, 5.00 L of N2 is saturated with water vapour at 22掳C and then compressed to half its volume at constant T.

(a) What is the partial pressure ofH2Oin the compressed gas mixture?

(b) What mass of water vapor condenses to liquid?

Short Answer

Expert verified
  1. The partial pressure of the moleculeH2Ois19.8torrat22oC.
  2. The mass of water vapor condenses to liquid is 720g.

Step by step solution

01

Formulas

The equation for the ideal gas is

PV=nRT

The moles are calculated as,

Number鈥�of鈥夆赌�Moles=MassMolarMass

02

Subpart (a) The partial pressure of H2O in the compressed gas mixture.

At temperature22掳C , the vapor pressure is 19.8torr.

The vapor pressure depends upon the temperature. Here, as the temperature is the same for the reaction, therefore the vapor pressure also remains the same.

03

Subpart (b) The mass of water vapor condenses to liquid.

Given,

Temperature 22掳C is equal to 295K.

Volume of the water 5L is 5000mL.

Gas Constant, R = 8.314 J/k/mole

Pressure at temperature role="math" localid="1658991569661" 22掳Cis 19.8torr.

Therefore, the number of moles of water at 22掳C:

PV=nRT19.8脳5000mL=n脳8.314脳295

And,

n=19.8脳5000mL8.314脳295n=40mole

The mass of the water moleculeat 22oC:

As,

Number鈥塷f鈥夆赌塎oles=MassMolarMass40=Mass18

Hence,

惭补蝉蝉=18脳40Mass=720g

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