If the total mass of the hydrogen in the hindenburg zeppelin was 18000kg, what volume did the hydrogen occupy?
To find the volume of the hydrogen in the Hindenburg zeppelin, we need to make use of the Ideal Gas Law equation. The Ideal Gas Law relates the pressure (P), volume (V), number of moles (n), and temperature (T) of a gas.
The formula for the Ideal Gas Law is:
PV = nRT
Where:
P = pressure (in Pascal, Pa)
V = volume (in cubic meters, m³)
n = number of moles
R = gas constant (typically 8.314 J/(mol·K))
T = temperature (in Kelvin, K)
Since we want to find the volume, we can rearrange the equation as follows:
V = (nRT) / P
In this case, we know the mass of the hydrogen (m = 18000 kg) and we can assume it is pure hydrogen (H₂). To find the number of moles, we can use the molar mass of hydrogen, which is approximately 2.016 g/mol.
Let's calculate the number of moles (n):
n = (mass of hydrogen) / (molar mass of hydrogen)
= (18000 kg) / (0.002016 kg/mol)
≈ 8928571 mol
Now, we need to assume a temperature and pressure for the gas. The temperature can be difficult to determine, as it would depend on the specific conditions during the Hindenburg zeppelin incident. However, we can use standard temperature and pressure (STP) conditions for a rough estimate. STP conditions are defined as 0 degrees Celsius (273.15 Kelvin) and 1 atmosphere of pressure (101325 Pascal).
Now, we can calculate the volume (V):
V = (nRT) / P
= [(8928571 mol) * (8.314 J/(mol·K)) * (273.15 K)] / (101325 Pa)
Calculating the volume gives us the answer.
2 grams of hydrogen occupies 22.4 litres,
so
18000kg=18000*1000 g will occupy
18000000/2*22.4 L
=9000 m³ (at STP)