Question

the good year blimp we usually see hovering sbove our heads at a football game contains 5500 m^3 of helium gas. If there are 1090 kg of gas at an absolute pressure of 1.10 x 10^5 Pa in the blimp, what is temperature of the gas? The atomic mass of helium 4.00260 g/mol.

_____________ K

Answer 1

Use the ideal gas equation to find temperature.

Ideal Gas equation:

PV = nRT

n = no. of moles of He

R = Gas constant

P = 1.10 * 10^5 Pa

V = 5500 m³

T = temperature

Now mass of gas = 1090 kg

Atomic mass of He = 4.00260 g / mole

So, 1 mole of He gas has mass = 4.0026 gm

or 1 gm has no. of moles = 1/4.0026 moles

thus no. of moles in 1090 kg = (1/4.0026) * 1090 * 1000 = 2.723*10^5 moles of He gas.

Now use the equation above:

PV = nRT

R = 8.314 J/mol K

Thus T = PV/nR

= 1.1 * 10^5 * 5500 / (2.723*10^5* 8.314)

T= 267.237 K

I hope help you !!