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A 40.0 L balloon is filled with air at sea level (1 atm @ 25 oC). It is then tied to a rock and thrown into a cold lake and it sinks to the bottom! When it reaches the bottom of the lake the temperature is 4.0 oC and the pressure has increased to 11 atm. What will the new volume be?
A. 0.295 L
B. 3.38 L
C. 3.91 L
D. 187.6 L

Answer :

To solve this question you need to calculate the number of the gas molecule. The calculation would be:
PV=nRT
n=PV/RT
n= 1 atm * 40 L/ (0.082 L atm mol-1K-1 * 298.15K)
n= 1.636 moles

The volume at bottom of the lake would be:
PV=nRT
V= nRT/P
V= (1.636 mol * 277.15K* 0.082 L atm mol-1K-1 )/ 11 atm= 3.38 L

The new volume of the ballon when thrown into a cold lake and it sinks to the bottom is 3.38 L.

How do we calculate volume?

Volume of the gas will be determined by using the ideal gas equation as:
PV = nRT

To calculate the volume first we calculate the moles of gas at sea level as:

P = pressure = 1 atm

V = volume = 40L

R = universal gas constant = 0.082 L.atm / mol.K

T = temperature = 25°C = 298.15K

Moles will be calculated by putting all these values on the above equation as:
n = (1)(40) / (0.082)(298.15) = 1.636 moles

Now we calculate the volume by putting values of moles and other details as:
P = pressure = 11 atm

V = volume = ?

R = universal gas constant = 0.082 L.atm / mol.K

T = temperature = 4°C = 277.15K

V = (1.636)(277.15)(0.082) / 11 = 3.38 L

Hence option (B) is correct i.e. 3.38 L.

To know more about ideal gas equation, visit the below link:
https://brainly.com/question/555495

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