Answer:
C.At the mountain top, the pressure inside the balloon is lower than at the new altitude.
Explanation:
The gas laws will come handy in predicting pressure, volume and temperature relationships of a given amount of gas.
Given parameters:
Volume at mountaintop = 5.0L
New volume at altitude = 25.0L
New pressure at altitude = 0.18atm
Pressure at mountaintop = ?
Here we are dealing with pressure and volume relationships between two given gases. The best law that gives a good prediction of what happen is the Boyle's law.
The law states that "the volume of a fixed mass(mole) of a gas varies inversely as the pressure changes, if the temperature is constant".
Mathematically;
P₁V₁ = P₂V₂
P₁ is the pressure at mountaintop
P₂ is the pressure at new altitude
V₁ is the volume at mountaintop
V₂ is the volume at new altitude.
From the definition of Boyle's law, we can clearly conclude that at the new altitude, the gas expands due to low pressure and will attain a new volume.
The pressure at mountaintop;
P₁ x 5 = 25 x 0.18
P₁ = 0.9atm
We can clearly see that at the mountaintop, the balloon has a higher pressure that confines the helium gas inside the balloon to a lower space.
An inverse relationship thus exists between volume and pressure
