Question

A helium filled weather balloon has a volume of 806 L at 20.9°C and 753 mmHg. it is released and rises to an altitude of 6.8 km, where the pressure is 417 mmHg and the temperature is -19.1°C what is the volume of the balloon

Answer 1

1257.45 L

Step-by-step explanation:

We are given;

• Initial volume of Helium gas, V1 as 806 L
• Initial temperature of Helium gas,T1 as 20.9°C
• Initial pressure of Helium gas, P1 as 753 mmHg
• Pressure of Helium at the altitude 6.8 km, P2 as 417 mmHg
• Temperature of Helium gas at the altitude 6.8 Km, T2 as -19.1°C

But, K = °C + 273.15

Therefore, T1 = 294.05 K and T2 = 254.05 K

• We are required to calculate the new volume of the balloon at 6.8 km.
• To determine the new volume we are going to use the combined gas law.
• According to the combined gas law,
  `(P1V1)/(T1)=(P2V2)/(T2)`

Thus, rearranging the formula;

`V2=(P1V1T2)/(P2T1)`

`V2=((753)(806L)(254.05K))/((417)(294.05))`

`V2=1257.45L`

Therefore, the volume of the balloon at an altitude of 6.8 km is 1257.45 L