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Chapter 6: Problem 48

How many liters of \(\mathrm{H}_{2}(\mathrm{g})\) at STP are produced per gram of \(\mathrm{Al}(\mathrm{s})\) consumed in the following reaction? \(2 \mathrm{Al}(\mathrm{s})+6 \mathrm{HCl}(\mathrm{aq}) \longrightarrow 2 \mathrm{AlCl}_{3}(\mathrm{aq})+3 \mathrm{H}_{2}(\mathrm{g})\)

Short Answer

Expert verified
The number of liters of \(\mathrm{H}_{2}\) gas produced per gram of \(\mathrm{Al}\) can be computed using the stoichiometry from the balance equation and molar volume at standard temperature and pressure (STP).

Step by step solution

01

Calculating moles of Aluminium

First, convert the mass of aluminium (Al) to moles using its molar mass (approximately 27.0 g/mol).
02

Using Stoichiometry

Next, use the balanced equation to find out how many moles of hydrogen are produced per mole of Al consumed: \[2 \mathrm{Al}(\mathrm{s})+6 \mathrm{HCl}(\mathrm{aq}) \longrightarrow 2 \mathrm{AlCl}_{3}(\mathrm{aq})+3 \mathrm{H}_{2}(\mathrm{g})\]. From this equation, you can see that 2 moles of Al produce 3 moles of H2. So, the stoichiometry yield is 3/2 moles of hydrogen for every mole of aluminium.
03

Convert moles of Hydrogen to volume

Convert the moles of hydrogen gas to liters using Avogadro set at standard temperature and pressure (STP), which is approximately 22.4 L/mol.

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Most popular questions from this chapter

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