Question

What is the minimum amount of 5.6 M H2SO4 necessary to produce 24.7 g of H2 (g) according to the following reaction? 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)

Answer 1

we have the Balanced chemical equation as:

2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g)

Molar mass of H2 = 2.016 g/mol

mass of H2 = 24.7 g

we have below equation to be used:

number of mol of H2,

n = mass of H2/molar mass of H2

=(24.7 g)/(2.016 g/mol)

= 12.25 mol

From balanced chemical reaction, we see that

when 3 mol of H2 forms, 3 mol of H2SO4 reacts

mol of H2SO4 reacted = (3/3)* moles of H2

= (3/3)*12.252

= 12.25 mol

This is number of moles of H2SO4

we have below equation to be used:

M = number of mol / volume in L

5.6 = 12.25/ volume in L

volume = 2.19 L

Answer: 2.19 L