Answer to Question #140308 in Molecular Physics | Thermodynamics for kayla

Question

The total mass of the hydrogen gas in the Hindenburg zeppelin was 18,000 kg. What volume did the hydrogen occupy? (Assume that the temperature of the hydrogen was 0°C and that it was at a pressure of 1 atm.)

Answer 1

Given,

Pressure, P = 1 atm

Temperature is 0°C

T = (0 +273)°C

= 273 K

Mass of Hydrogen,W = 18000 kg

= 18000 x 10³ g

(Since, 1kg = 10³ g)

Molar mass of Hydrogen, M = 2 g/mole

Number of moles of Hydrogen,

n = (W/M)

Or, n = (18000x10³/2) mole

Or, n = 9x10⁶ mole

Taking ideal gas behaviour,

We can use Idea gas equation

PV = nRT.

(R= universal gas constant

= 0.082 liter.atm)

Or, V = (nRT/P)

Putting the values,

Or, V =(9x10⁶ x0.082 x273/1)

Or, V = 201.474x10⁶

Hence the volume occupied by the given amount of Hydrogen gas = 201.474x10⁶ liter