Question

The total volume of hydrogen gas needed to fill the hindenburg was 2.09 × 108 l at 1.00 atm and 25.1°

Answer 1

The solution for this problem:

PV = nRT 

But we are looking for n so, alter the original formula:
n = PV / RT

= (1.00 atm) x (2.09 x 10^8 L) / ((0.08205746 L atm/K mol) x  (25.1 + 273.15 K)) 

= 8539801.26 mol H2 
total volume = (8539801.26 mol H2) x (-286 kJ/mol H2) = -2.44 x 10^9 k J

Answer 2

Answer:$2.4453\times 10^9 kJ$  energy was evolved when it burned.

Explanation:

Volume of the hydrogen gas = $2.09\times 10^{8} L$

Pressure of the gas = P = 1 atm

Temperature of the gas =T = 25.1 °C =298.1 K[/tex]

$PV=nRT$

$1 atm\times 2.09\times 10^{8} L=n\times 0.0820 atm L/mol K\times 298.1 K$

$n=\frac{1 atm\times 2.09\times 10^{8} L}{0.0820 atm L/mol K\times 298.1 K}=0.0855\times 10^8 mol$

$\Delta H_{C}$ for hydrogen gas=-286 kJ/mol

For $0.0855\times 10^8 mol$ energy evolved when hydrogen gas is burned =$0.0855 mol\times (-286 kJ/mol)=-2.4453\times 10^9 kJ$

$2.4453\times 10^9 kJ$  energy was evolved when it burned.