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Chapter 5: Q5.12P (page 227)

If the sample flask in Figure P5.12 is open to the air, what is the atmospheric pressure (in atm)?

Short Answer

Expert verified

The atmospheric pressure is 0.966 atm.

Step by step solution

01

Determination of the atmospheric pressure

The atmospheric pressure is equal to the difference in height of the mercury column.

∆h = Patmospheric

Now, height is,

∆h = 0.734 m

Convert m into mm,

    1.0 m = 1000 mm⇒ 0.734 m = 734  mm

So, the atmospheric pressure is 734 mmHg.

02

Conversion of unit from mmHg to atm 

1 atm = 760 mmHg

Now, the pressure is,

734 mmHg × 1 atm760 mmHg  = 0.966  atm

Thus, the atmospheric pressure is 0.966 atm.

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Most popular questions from this chapter

What is the pressure (in Pa) of the gas in the flask in Figure P5.13?

How does a sample of gas differ in its behavior from a sample of liquid in each of the following situations?

(a) The sample is transferred from one container to a larger one.

(b) The sample is heated in an expandable container, but no change of state occurs.

(c) The sample is placed in a cylinder with a piston, and an external force is applied.

What is the effect of the following on the volume of 1 mol of an ideal gas?

(a) Half the gas escapes (at constantPandT).

(b) The initial pressure is 722 torr, and the final pressure is 0.950 atm; the initial temperature is 32oF, and the final temperature is 273 K.

(c) Both the pressure and temperature decrease to one-fourth of their initial values.

The gravitational force exerted by an object is given by F= mg,where Fis the force in Newtons, mis the mass in kilograms, and gis the acceleration due to gravity (9.81 m/s2).

(a) Use the definition of the pascal to calculate the mass (in kg) of the atmosphere above 1 m2 of ocean.

(b) Osmium (Z= 76) is a transition metal in Group 8B(8) and has the highest density of any element (22.6 g/mL). If an osmium column is 1 m2 in area, how high must it be for its pressure to equal atmospheric pressure? [Use the answer from part (a) in your calculation.]

A sample of chlorine gas is confined in a 5.0-L container at 328 torr and 37°C. How many moles of gas are in the sample?
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