How to Calculate the Volume of a Helium Balloon at Different Altitudes?
What is the initial pressure, volume, and temperature of the helium balloon?
The initial pressure of the helium balloon is 1.25 atm, the volume is 3.50 L, and the temperature is 25.00°C.
What altitude has a pressure of 0.800 atm and a temperature of -30.00°C?
The altitude where the pressure is 0.800 atm and the temperature is -30.00°C.
How do you calculate the volume of the balloon at the different altitude?
Using the combined gas law ((P1•V1)/T1) = ((P2•V2)/T2) to find the volume of the balloon at the different altitude.
Answer:
The volume of the helium balloon at the different altitude can be calculated using the combined gas law equation:
((P1•V1)/T1) = ((P2•V2)/T2)
Substitute the initial values P1 = 1.25 atm, V1 = 3.50 L, and T1 = 25.00°C, along with the altitude values P2 = 0.800 atm and T2 = -30.00°C into the equation.
After solving for V2, you will get the volume of the balloon at the different altitude, which is 4.46 L.
Imagine releasing a helium balloon into the sky and watching it float away! As the balloon ascends to different altitudes, the pressure and temperature around it change, affecting its volume. In this scenario, we have an initial helium balloon with a pressure of 1.25 atm, a volume of 3.50 L, and a temperature of 25.00°C.
Now, let's calculate the volume of the balloon when it reaches an altitude where the pressure is 0.800 atm and the temperature is -30.00°C. By using the combined gas law formula ((P1•V1)/T1) = ((P2•V2)/T2), we can determine the final volume of the balloon at the new altitude.
Substitute the initial values into the equation: ((1.25 atm • 3.50 L) / 298 K) = ((0.800 atm • V2) / 243 K). Solve for V2 to find that the balloon will occupy 4.46 L at the new altitude. Isn't it amazing to see how changes in pressure and temperature can affect the volume of a helium balloon?