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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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