I have no clue how to figure this problem out..
The Goodyear blimps, which frequently fly over sporting events, hold approximately 1.90×105 ft^3 of helium. If the gas is at 24 degrees Celsius and 1.0 atm, what mass of helium is in the blimp?
PV=mass/molmassHe * RT
solve for mass.
I would start by changing ft^3 to m^3
To determine the mass of helium in the blimp, we can use the Ideal Gas Law, which states:
PV = nRT
Where:
P = pressure (in atmospheres)
V = volume (in liters)
n = number of moles
R = ideal gas constant (0.0821 L·atm/(mol·K))
T = temperature (in Kelvin)
Let's go through the steps to solve this problem:
1. Convert the given volume from cubic feet (ft^3) to liters (L). To do this, we can use the conversion factor:
1 ft^3 ≈ 28.32 L
So, 1.90×10^5 ft^3 ≈ 1.90×10^5 * 28.32 L ≈ 5.39×10^6 L
2. Convert the temperature from degrees Celsius to Kelvin. To do this, we use the formula:
T(K) = T(°C) + 273.15
So, 24°C + 273.15 = 297.15 K
3. Substitute the values into the Ideal Gas Law equation and solve for n (number of moles):
PV = nRT
1.0 atm * 5.39×10^6 L = n * 0.0821 L·atm/(mol·K) * 297.15 K
Solving for n:
n = (1.0 atm * 5.39×10^6 L) / (0.0821 L·atm/(mol·K) * 297.15 K)
4. Calculate the number of moles of helium in the blimp.
5. Use the molar mass of helium to convert moles to grams. The molar mass of helium (He) is approximately 4.00 g/mol.
6. Calculate the mass using the formula:
mass = moles * molar mass
By following these steps, you should be able to find the mass of helium in the blimp.