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Chapter 5: Q5.10P (page 227)

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

Short Answer

Expert verified

The pressure of the gas is 0.941 atm.

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 the total pressure from torr to mmHg.

鈥�鈥�鈥�鈥�1鈥�torr鈥�=鈥�1鈥�mmHg鈬�738.5鈥�torr鈥�= 738.5鈥�mmHg

Convert cmHg to mmHg

鈥�鈥�1鈥�cmHg鈥�=鈥�10鈥�mmHg鈬�2.35鈥�cmHg鈥�=鈥�23.5鈥�mmHg

Now, the pressure of the gas is,

Ptotal=鈭唄+笔gasPgas鈥�=鈥�Ptotal鈥�鈥�-鈭唄= 738.5鈥�mmHg鈥�-鈥�23.5鈥�鈥�mmHg=鈥�鈥�715鈥�mmHg

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

1 atm = 760 mmHg

715鈥�mmHg鈥�鈥�脳1鈥�atm760鈥�鈥�mmHg鈥�=鈥�0.941鈥�atm

Thus, the pressure of the gas is 0.941 atm.

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Most popular questions from this chapter

Each of the following processes caused the gas volume to double, as shown. For each process, state how the remaining gas variable changed or that it remained fixed:

(a)Tdoubles at fixedP.

(b)Tandnare fixed.

(c) At fixed T, the reaction is CD2(g)鈫�C(g)+D2(g)

(d) At fixed P, the reaction is A2(g)+B2(g)鈫�2AB(g)

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

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.

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

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

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