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Chapter 5: Q5.11P (page 227)

In Figure P5.11, what is the pressure of the gas in the flask (in kPa) if the barometer reads 765.2 mmHg?

Short Answer

Expert verified

The pressure of the gas is 100.0 kPa.

Step by step solution

01

Total pressure

Total pressure is the sum of the pressure of the atmosphere and the difference in heights of the columns.

02

Determination of pressure of the gas

Convert cmHg to mmHg

       1 cmHg = 10 mmHg⇒1.3 cmHg = 13 mmHg

The pressure of the gas is,

Ptotal=∆h+ PgasPgas = Ptotal  -∆h= 765.2 mmHg - 13  mmHg=  752.2 mmHg

Now, convert the pressure of the gas from mmHg to kPa,

1 mmHg = 0.133 kPa

752.2 mmHg×0.133 kPa1  mmHg = 100.0 kPa

Thus, the pressure of the gas is 100.0 kPa.

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Most popular questions from this chapter

How does a barometer work? Is the column of mercury in a barometer shorter when it is on a mountaintop or at sea level? Explain.

In a closed-end manometer, the mercury level in the arm attached to the flask can never be higher than the mercury level in the other arm, whereas in an open-end manometer, it can be higher. Explain.

How can a unit of length such as millimetre of mercury (mmHg) be used as a unit of pressure, which has the dimensions of force per unit area?

A sample of sulfur hexafluoride gas occupies 9.10 L at 198°C. Assuming that the pressure remains constant, what temperature (in °C) is needed to reduce the volume to 2.50 L?

Convert the following:

(a) 76.8 cmHg to atm (b) 27.5 atm to kPa

(c) 6.50 atm to bar (d) 0.937 kPa to torr
See all solutions

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