A Goodyear blimp typically contains 5040 m3 of helium (He) at an absolute pressure of 1.10 x 105 Pa. The temperature of the helium is 282 K. What is the mass (in kg) of the helium in the blimp?

To determine the mass of helium in the blimp, we can use the ideal gas law equation:

PV = nRT

Where:
P = absolute pressure (in Pa)
V = volume (in m^3)
n = number of moles
R = ideal gas constant (8.314 J/(mol·K))
T = temperature (in K)

We can rearrange the equation to solve for the number of moles:

n = PV / RT

Given:
P = 1.10 x 10^5 Pa
V = 5040 m^3
T = 282 K

Substituting the values into the equation:

n = (1.10 x 10^5 Pa) * (5040 m^3) / ((8.314 J/(mol·K)) * (282 K))

Calculating this:

n ≈ 266.62 mol

Now, to find the mass of helium in kg, we need to multiply the number of moles by the molar mass of helium (He), which is 4.0026 g/mol (or 0.0040026 kg/mol):

Mass = n * molar mass

Mass = (266.62 mol) * (0.0040026 kg/mol)

Calculating this:

Mass ≈ 1.067 kg

Therefore, the mass of helium in the blimp is approximately 1.067 kg.