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Chapter 5: Q5.13P (page 227)

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

Short Answer

Expert verified

The pressure of the gas is 4.75×10 3 Pa.

Step by step solution

01

Determination of the pressure 

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

∆h =Pgas

Now, the difference in height of the mercury column is :

∆h = 3.56 cm

Convert m into mm,

      1 cmHg = 10 mmHg⇒3.56 cmHg = 35.6 mmHg

So, the pressure is 35.6 mmHg.
02

Conversion of unit from mmHg to Pascal (Pa) 

1 mmHg = 133.322 Pa

Now, the pressure is,

35.6 mmHg  ×133.322 Pa1  mmHg  =  4.75×103 Pa

Thus, the pressure of the gas is 4.75 ×10 3 Pa.

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Most popular questions from this chapter

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

(a) Temperature decreases from 800 K to 400 K (at constantP).

(b) Temperature increases from 250°Cto 500°C(at constantP).

(c) Pressure increases from 2 atm to 6 atm (at constant T).

In Figure P5.10, what is the pressure of the gas in the flask (in atm) if the barometer reads 738.5 torr?

A gas-filled weather balloon with a volume of 65.0 L is released at sea-level conditions of 745 torr and 25°C. The balloon can expand to a maximum volume of 835 L. When the balloon rises to an altitude at which the temperature is−5°C and the pressure is 0.066 atm, will it reach its maximum volume?

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

(a) The pressure is tripled (at constantT).

(b) The absolute temperature is increased by a factor of 3.0 (at constantP).

(c) Three more moles of the gas are added (at constant P and T).

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?
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