A small piece of pure Al Metal having a volume of 2.50 cm3 is reacted with excess
density
of HCI. What is the weight of H2 liberated? The density of Al is 2.70 g cm3
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Concept:
The ratio of mass to volume can be defined as Density.
d = m/V
Given:
The volume of the Al metal, V = 2.50 cm³
The density of Al, d = 2.70 g/cm³
Find:
Weight of the hydrogen, H₂ liberated.
Solution:
Mass of the aluminum can be calculated,
d = m/V
m = d×V
m = (2.50)×(2.70)
m = 6.75 g of Aluminum
No. of moles of the Aluminium, n = Mass/Molar mass
n = 6.75/27 = 0.25 moles
The reaction can be written as,
Al + HCl → AlCl₃ + H₂
The number of moles of aluminum equals the number of moles of hydrogen liberated.
The molar mass of the hydrogen is 2 g/mol.
Moles of the hydrogen are 0.25 moles.
n = mass/Molar mass
mass, m = n × M
m = 0.25 × 2 = 0.5 g
Hence, the weight of the hydrogen, H₂ liberated is 0.5 g.
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