the hindenburg was a hydrogen -filled dirigiable that exploded on 1937. The Hindenburg held 6.5*10^5 L of hydrogen gas at 23C and 760mmHg, what mass of hydrogen (H2) was present?
calculate n in PV=nRT
mass=n*molmassH2
To calculate the mass of hydrogen (H2) present in the Hindenburg, we need to use the ideal gas law equation PV = nRT. Here's how you can approach the problem:
Step 1: Identify the given values:
- Volume (V) = 6.5 × 10^5 L
- Pressure (P) = 760 mmHg (which is equivalent to 1 atm)
- Temperature (T) = 23°C (which needs to be converted to Kelvin: T = 23 + 273 = 296 K)
- Universal gas constant (R) = 0.0821 L·atm/(mol·K) (this value is commonly used, but make sure to check if your textbook or teacher specifies a different value)
Step 2: Plug the values into the ideal gas law equation:
PV = nRT
n = (PV) / (RT)
Substitute the values:
n = (1 atm) × (6.5 × 10^5 L) / (0.0821 L·atm/(mol·K) × 296 K)
Step 3: Calculate the value of n:
n ≈ 27965.179 mol
Step 4: Calculate the mass of hydrogen (H2):
mass = n × mol mass of H2
The molar mass of hydrogen (H2) is approximately 2 g/mol. Therefore:
mass = (27965.179 mol) × (2 g/mol)
mass ≈ 55930.358 g
So, the mass of hydrogen (H2) present in the Hindenburg is approximately 55930.358 grams.