
Concept explainers
A 3.00-L flask containing 2.0 mol of O2 and 1.0 mol of N2 is in a room that is at 22.0°C.
- a How much (what fraction) of the total pressure in the flask is due to the N2?
- b The flask is cooled and the pressure drops. What happens, if anything, to the mole fraction of the O2 at the lower temperature?
- c L of liquid water is introduced into the flask containing both gases. The pressure is then measured about 45 minutes later. Would you expect the measured pressure to be higher or lower?
- d Given the information in this problem and the conditions in part c, would it be possible to calculate the pressure in the flask after the introduction of the water? If it is not possible with the given information, what further information would you need to accomplish this task?
(a)

Interpretation:
The amount of pressure due to N2 gas present in a 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 should be measured.
Concept Introduction:
Ideal gas equation:
At a constant temperature (K) and pressure (P), the volume (v) occupied by the no of moles of any gas is known as ideal gas equation.
Ideal gas equation:
And the SI units are
Answer to Problem 5.32QP
The total pressure fraction due to N2 gas is
Explanation of Solution
The flask contains 1.0 mol of N2 gas out of 3.0 mol container, so the fraction of N2 gas in the container is
The amount of pressure due to N2 gas present in a 3.00 L flask containing 2.0 mol of O2 and 1.0 mol of N2 was measured.
(b)

Interpretation:
The change in mole fraction of O2 at lower temperature in the flask should be explained
Concept Introduction:
Ideal gas equation:
At a constant temperature (K) and pressure (P), the volume (v) occupied by the no of moles of any gas is known as ideal gas equation.
Ideal gas equation:
And the SI units are
Answer to Problem 5.32QP
There will be no change in mole fraction of
Explanation of Solution
From the ideal gas equation,
The change in mole fraction of O2 at lower temperature in the flask was explained.
(c)

Interpretation:
The change in pressure when the 1.0 L liquid water added to the flask containing two gases should be explained.
Concept Introduction:
Ideal gas equation:
At a constant temperature (K) and pressure (P), the volume (v) occupied by the no of moles of any gas is known as ideal gas equation.
Ideal gas equation:
And the SI units are
Answer to Problem 5.32QP
Explanation of Solution
According to ideal gas equation, the pressure in the flask is increases for two reasons
- 1. When the water enters the flask occupies some spaces occupied by the gas earlier making gas molecules increase in pressure.
- 2. When the liquid water enters the flask it would evaporate after a time, and evaporate water would contribute the increase in pressure.
The change in pressure when the 1.0 L liquid water added to the flask containing two gases was explained.
(d)

Interpretation:
Using the parameters given in the part c is it possible to calculate the change in pressure should be explained.
Concept Introduction:
Ideal gas equation:
At a constant temperature (K) and pressure (P), the volume (v) occupied by the no of moles of any gas is known as ideal gas equation.
Ideal gas equation:
And the SI units are
Answer to Problem 5.32QP
Explanation of Solution
For calculating pressure from ideal gas equation, we have to know the volume and temperature of the given gas. As the volume of the flask is fixed and temperature is lowered and it can be measured and the gas constant “R’’ value we knew it is a constant and the value of water vapor pressure should be known so that we can calculate the pressure in the flask.
The change in pressure when the 1.0 L liquid water added to the flask containing two gases was explained.
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