Question

What is the mass of Al required to produce 4.0g of hydrogen according to the equation?
2Al + 3H2SO4 = Al2(SO4)3

Answer 1

Given:  The equation given is  2Al+3H2SO4=Al2(SO4)3

             Amount of Hydrogen to be prepared =4gm

To Find: Mass of Aluminium(Al) required to produce 4gm of Hydrogen

Solution:  According to the given equation 2 moles of Aluminium (Al) is reacting with 3 moles of Hydrogen(H2)

Number of moles of Al= Given weight of Al/Gram molecular weight

The gram molecular weight of Al=44g

2=Given weight of Al/27

The weight of Al=27x2

                           =54grams

Number of moles of H2=Given weight of H2 /Gram molecular weight of H2

The gram molecular weight of H2=2 grams

3=Given weight of H2/2

The weight of H2=6grams

54grams of Al reacts with 6 grams of H2

Amount of Al reacting with 4grams of H2 = 4x54/6

=36grams

The mass of Al required to produce 4 grams of H2 is 36 grams