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I have a special ideal balloon. This balloon does not exert any pressure on the gas inside it. I started by taking the balloon and inflating it to 4 L on Brooklyn Ny last night. The weather channel said that the temperature was 45.0 degree Celsius, and the pressure was 50.27 mm of Hg.

First i took this balloon scuba diving and went down to a depth of 100 ft where the pressure is 7 atm. And the temperature is 52.2 Celsius. What is the volume of the balloon?

Verified Answer :

MissPhiladelphia

Using ideal gas law

PV = nRT

Where p is pressure

V is the volume

n is the number of moles

R is the gas constant

T is the temperature

First solve for the number of moles



N = (50.27 mmHg) ( 4 L) / [( 760 mmHg)( 22.414 L/mol)/
273.15 K)] ( 45 + 273.15 K)


N = 0.01013 moles



Then solving for the volume

V = nRT / P

V =  0.01013 moles [ ( 1 atm)( 22.414 L/mol)/ 273.15 K)] ( 52.2 +
273.15 K) / 7 atm


V = 0.03865 L

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