Answer:
102.26 moles of helium were required to Fill the Goodyear Blimp
Explanation:
To solve this question we need to use combined gas law:
PV = nRT
Where P is pressure, V is volume of gas (2500L), n are moles of gas (Our incognite), R is gas constant (0.082atmL/molK) and T is absolute temperature
Assuming atmospheric condition we can write P = 1atm and T = 25°C = 298.15K
Replacing:
PV/RT = n
1atm*2500L / 0.082atmL/molK*298.15K = n
102.26 moles of helium were required to Fill the Goodyear Blimp
