Question

What is the minimum amount of 5.3 M H2SO4 necessary to produce 22.0 g of H2...

What is the minimum amount of 5.3 M H2SO4 necessary to produce 22.0 g of H2 (g) according to the following reaction? 2Al(s)+3H2SO4(aq)→Al2(SO4)3(aq)+3H2(g) Express your answer using two significant figures.

Homework Answers

Answer #1

Molar mass of H2 = 2.016 g/mol

mass of H2 = 22.0 g

we have below equation to be used:

number of mol of H2,

n = mass of H2/molar mass of H2

=(22.0 g)/(2.016 g/mol)

= 10.91 mol

From balanced chemical reaction, we see that

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

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

= (3/3)*10.9127

= 10.91 mol

This is number of moles of H2SO4

we have below equation to be used:

M = number of mol / volume in L

5.3 = 10.91/ volume in L

volume = 2.1 L

Answer: 2.1 L

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