In 1793 the French physicist Jacques Charles took part in the first recorded human flight in a Hydrogen balloon. The Hydrogen was produced by reacting iron filings with sulfuric acid to yield hydrogen gas and Iron(II) sulfate. What volume (in L) of Hydrogen gas at 22.0 °C and 756 mm Hg will be formed from the reaction of 500.0 gallons of 12.0 M sulfuric acid according to the following equation:
reaction is
Fe + H2SO4 ----> FeSO4 + H2
1 mole 1mole 1mole 1 mole
Given
T = 22 C = 295 K
P = 756 mmHg = 0.995 atm
Given
reaction mixture volume = 500 gallons = 500 * 3.7854 L = 1892.7 L
Molarity of sulfuric acid = 12 M (mol/L)
No. of moles of sulfuric acid = Molarity * volume of reaction mixture = 12 mol/L * 1892.7 L =22712.4 moles
For every mole of sullfuric acid reacted one mole of H2 is formed
so no. of moles of H2 formed n = 22712.4 moles
R = 0.08206 L.atm/mol.K
PV = nRT
0.995 atm * V = 22712.4 mol * 0.08206 L.atm/mol.K * 295 K
V = 552577.855 L Answer
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