A Goodyear blimp typically contains 4770 m3 of helium (He) at an absolute pressure of 1.10 x 105 Pa. The temperature of the helium is 274 K. What is the mass (in kg) of the helium in the blimp?

A Goodyear blimp typically contains 4770 m3 of helium (He) at an absolute pressure of 1.10 x 105 Pa. The temperature of the helium is 274 K. What is the mass (in kg) of the helium in the blimp?

Explain Bot Explain Bot answered
8 months ago

To find the mass of the helium in the blimp, we can use the ideal gas equation, which states:

PV = nRT

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

First, we need to calculate the number of moles of helium using the ideal gas equation. Rearranging the equation, we have:

n = PV / RT

Given:
P = 1.10 x 10^5 Pa
V = 4770 m^3
R = 8.314 J/(mol·K)
T = 274 K

Let's plug in the values and solve for n:

n = (1.10 x 10^5 Pa) * (4770 m^3) / (8.314 J/(mol·K) * 274 K)

Calculating this expression will give us the number of moles of helium.

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