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

Answer:

1257.45 L

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, $\frac{P1V1}{T1}=\frac{P2V2}{T2}$

Thus, rearranging the formula;

$V2=\frac{P1V1T2}{P2T1}$

$V2=\frac{(753)(806L)(254.05K)}{(417)(294.05)}$

$V2=1257.45L$

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