Ahelium 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

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°CInitial 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,

Thus, rearranging the formula;

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

Idk the answer sorry