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?
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.