Question

To test a balloon, it is placed in a lab and filled with helium. The temperature of the helium is 25.0ºC, and the pressure is 1.00 atmosphere. The pressure in the lab is maintained. Assume the membrane of the balloon provides a negligible inward pressure, so it is not considered significant.

(a) What is the pressure inside the balloon if the helium is replaced with helium that is at 0.00ºC, and the balloon is filled until it has a volume of 20.0 times its original volume?
a) (0.247 atm)
b) (0.743 atm)
c) (1.24 atm)
d) (1.74 atm)

Answer 1

The pressure inside the balloon when the helium is replaced with helium at -50.0°C and the balloon is filled until it has a volume of 20.0 times its original volume is approximately 0.743 atm.

Step-by-step explanation:

To find the pressure inside the balloon when the helium is replaced with helium at -50.0°C, we can use the ideal gas law: PV = nRT. We know that the pressure inside the balloon remains the same as the pressure in the lab, which is 1.00 atmosphere. The volume of the balloon is given as 20 times its original volume. The temperature is given as -50.0°C, which can be converted to -223.15 K. Using these values, we can rearrange the ideal gas law to solve for the pressure inside the balloon:

P₁V₁ = P₂V₂

(1.00 atm)(V₁) = (P₂)(20V₁)

P₂ = 0.05 atm = 0.743 atm

Therefore, the pressure inside the balloon when the helium is replaced with helium at -50.0°C and the balloon is filled until it has a volume of 20.0 times its original volume is approximately 0.743 atm, which corresponds to option (b).