Chapter 21, Problem 52PS

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074

Chapter
Section

### Chemistry & Chemical Reactivity

10th Edition
John C. Kotz + 3 others
ISBN: 9781337399074
Textbook Problem

# “Aerated” concrete bricks are widely used building materials. They are obtained by mixing gas-forming additives with a moist mixture of lime, cement, and possibly sand. Industrially, the following reaction is important: 2  Al(s) + 3 Ca(OH) 2 ( s ) + 6  H 2 O( l )  → 3  CaO ⋅ Al 2 O 3 ⋅ 6  H 2 O(s) + 3 H 2 ( g ) Assume the mixture of reactants contains 0.56 g of Al (as well as excess calcium hydroxide and water) for each brick. What volume of hydrogen gas do you expect at 26°C and a pressure of 745 mm Hg?

Interpretation Introduction

Interpretation:

To and predict the volume of H2 gas produced at the given temperature and pressure.

Concept introduction:

Aluminium belongs to group 3A of the periodic table. It react with a base like calcium hydroxide and water to produce aerated concrete bricks and hydrogen gas. The aerated concrete brick formed has the chemical formula of CaOAl2O36H2O.

The balanced chemical equation is,

2Al(s)+3Ca(OH)2(s)+6H2O(l)3CaOAl2O36H2O(s)+3H2(g)

Ideal gas equation is,

PV=nRT

Where P, V, T, n, and R are the pressure, volume, temperature and amount of substance respectively.

Explanation

The volume of H2 gas produced from 0.56Â g of Aluminium is calculated below.

Given,

The balanced chemical equation is,

Â Â Â Â 2Al(s)+3Ca(OH)2(s)+6H2O(l)â†’3CaOâ‹…Al2O3â‹…6H2O(s)+3H2(g)

The molar mass of aluminium is 27Â g. The mass of two moles of Aluminium is 54Â g.

Two moles of aluminium is forming three moles of hydrogen.

Volume of gas produced at given temperature of 299Â K and pressure of 745Â mmHg can be calculated as follows,

Vmolar=(299Â K)(0

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