Question

The Goodyear blimp contains 5.7 x 10^6 L of helium at 25 degrees Celsius and 1 atm. What is the mass in grams of the helium inside the blimp

Answer 1

1.72x10⁻⁵ g

Step-by-step explanation:

To solve this problem we use the PV=nRT equation, where:

• P = 1 atm

• V = 5.7x10⁶ L

• n = ?

• R = 0.082 atm·L·mol⁻¹·K⁻¹

• T = 25 °C ⇒ (25+273.16) = 298.16 K

And we solve for n:

• 1 atm * 5.7x10⁶ L = n * 0.082 atm·L·mol⁻¹·K⁻¹ * 298.16 K

• n = 4.29x10⁻⁶ mol

Finally we convert moles of helium to grams, using its molar mass:

• 4.29x10⁻⁶ mol * 4 g/mol = 1.72x10⁻⁵ g