1. Calculate the pressure (in atm) of a sample of gas collected over water at 40

Question

1. Calculate the pressure (in atm) of a sample of gas collected over water at 40oC if the atmospheric pressure is 758.2 mm Hg. Remember, 1 atm = 760 mm Hg and Table 11.3 in the textbook gives the vapor pressure of water as a function of temperature.

2. In Part II of this experiment, you will be measuring the volume of trapped air in an inverted graduated cylinder in a hot water bath. This air will be mixed with water vapor from the bath. The barometric pressure in the laboratory is 0.989 atm. What is the volume of dry air in mL if you record a total volume of 7.8 mL at a temperature where the vapor pressure of water is 0.052 atm?

3. A graph of a set of data reveals a linear relationship between two variables. The best fit equation is y = 0.198x + 6.75. Determine the value of the x-intercept for this line.

Hint- Do not confuse x-intercept with y-intercept

Explanation / Answer

ANSWER

Dear candidate you have asked three different questions. As per guidelines one question one time. All the same here we solve first two questions. Pleasesnt 3rd separately.

1) CONCEPT: The first two question are based on Daltons Law of partial pressures

Ptotal = Pdry gas + Pwater

Pdry gas = Ptotal - Pwater

Pdry gas = 758.2 -   55.3 = 702.9mmHg   

Vapour pressure of water at 40C = 55.3mmHg, if not Please confirm from your text book as it is mentioned in question

pressure in atm units = 702.9/760 = 0.925atm

2) given conditions

V1 = 7.8mL

P1 = 0.989 - 0.052 = 0.937atm

here T1 = T2

V2 = ?

P2 = 1atm (Atmospheric pressure)

P1V1 = P2V2

V2 = P1V1/P2 = 0.937 X 7.8/1 = 7.31mL

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