Question

The Goodyear blimp we usually see hovering above our heads at a football game contains 5600 m3 of helium gas. If there are 1070 kg of gas at an absolute pressure of 1.10 105 Pa in the blimp, what is the temperature of the gas? The atomic mass of helium 4.00260 g/mol.

Answer 1

Answer:

277.16 K is the temperature of the gas.

Explanation:

Using ideal gas equation:

PV = nRT

where,

P = Pressure of gas = $1.10\times 10^5 Pa$

V = Volume of gas = $5600 m^3$

n = number of moles of gas = $\frac{1,070 kg}{4.00260 g/mol}=\frac{1,070,000 g}{4.00260 g/mol}=267,326.24 mol$

R = Gas constant = 8.314 J/mol.K

T = Temperature of gas = ?

Putting values in above equation, we get:

$T=\frac{PV}{RT}$

$T=\frac{1.10\times 10^5 Pa\times 5,600 m^3}{267,326.24 mol\times 8.314 J/mol K}$

T = 277.16 K

277.16 K is the temperature of the gas.