A Goodyear blimp typically contains 5400m^3 of helium (He) at an absolute pressure of 1.1*10^5Pa. The temperature of the helium is 280K. What is the mass (in kg)of the helium in the blimp?

PLEASE GIVE ME SOME IDEAS TO DO IT!!!THANKS A LOT!!!

I would find an equation to fit this question.

I know that I should find an equation, but which one?

P V = n R T

that gives you the moles of He

each mole has mass of 4 grams or 4*10^-3 kg

To calculate the mass of the helium in the blimp, you can use the ideal gas law equation: PV = nRT.

First, we need to convert the volume from cubic meters to liters. Since 1 cubic meter is equal to 1000 liters, the volume of the blimp is 5400 m^3 * 1000 L/m^3 = 5,400,000 L.

Now, let's rearrange the ideal gas law equation to solve for the number of moles (n):
n = PV / RT

Where:
P = absolute pressure = 1.1 * 10^5 Pa
V = volume = 5,400,000 L = 5,400,000 dm^3 (since 1 L = 1 dm^3)
R = ideal gas constant = 8.314 J/(mol·K)
T = temperature in Kelvin = 280 K

Substituting these values, we get:
n = (1.1 * 10^5 Pa) * (5,400,000 dm^3) / (8.314 J/(mol·K) * 280 K)

Now, calculate the value for n.

Once you have the number of moles (n) of helium, you can calculate the mass using the molar mass of helium. The molar mass of helium (He) is approximately 4 g/mol.

Finally, multiply the number of moles by the molar mass to find the mass of the helium in the blimp in grams. Remember to convert from grams to kilograms by dividing the result by 1000.

I hope this helps you solve the problem!