A balloon is filled with gas at a pressure of 102.3 Kpa and a temperature of 45.5°C. It's volume under these conditions is 12.5L. The balloon is then taken into a decompression chamber where the volume is measured as 2.50L. If the temperature is 36.0°C, what is the pressure in the chamber?

496.24 KPa

Explanation:

Step 1:

Data obtained from the question.

Initial pressure (P1) = 102.3 KPa

Initial temperature (T1) = 45.5°C = 45.5°C + 273 = 318.5K

Initial volume (V1) = 12.5L

Final volume (V2) = 2.50L

Final temperature (T2) = 36.0°C = 36.0°C + 273 = 309K

Final pressure (P2) =?

Step 2:

Determination of the pressure in the chamber.

The final pressure i.e the pressure of the chamber can be obtained by using the general gas equation as follow:

P1V1/T1 = P2V2/T2

102.3 x 12.5/318.5 = P2 x 2.5/309

Cross multiply to express in linear form

318.5 x 2.5 x P2 = 102.3 x 12.5 x 309

Divide both side by (318.5 x 2.5)

P2 = (102.3 x 12.5 x 309)/(318.5x2.5)

P2 = 496.24 KPa

Therefore, the pressure in the chamber is 496.24 KPa

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