Question

1) N2(g) + 3H2(g) 2NH3(g)

2) 4NH3(g) + 5O2(g) 4NO(g) + 6H2O(g)

3) 2NO(g) + O2(g) 2NO2(g)

What mass of hydrogen gas is needed to produce 147.0 kg of nitrogen dioxide?

Answer 1

From the above three equations:

2 mole of NO2 is formed from 2 moles of NO (equation 3)

2 mole of NO can be formed from 2 moles of NH3

2 moles of NH3 can be formed from 3/2 moles of H2

So, 2 moles of NO2 can be formed from 3/2 moles of H2

Molar masss of NO2 = 46.01 g/mol

Molar mass of H2 = 2.02 g/mol

Since, Amount of H2 reaquired for the synthesis of 2 x 46.01 g NO2 synthesis = 3/2 x 2.02 g

So, Amount of H2 reaquired for the synthesis of 147 Kg (147000 g) NO2 synthesis

= (3/2 x 2.02 x 147000) /2 x 46.01

= 4840.36 g

= 4.84 Kg