   Chapter 18, Problem 21Q

Chapter
Section
Textbook Problem

# When magnesium metal is added to a beaker of HCl(aq), a gas is produced. Knowing that magnesium is oxidized and that hydrogen is reduced, write the balanced equation for the reaction. How many electrons are transferred in the balanced equation? What quantity of useful work can be obtained when Mg is added directly to the beaker of HCl? How can you harness this reaction to do useful work?

Interpretation Introduction

Interpretation:

The production of a gas on addition of magnesium metal to a beaker of HCl(aq) and the species undergoing oxidation and reduction reactions are given. The balanced chemical equation, the number of electrons transferred, amount of useful work that can be obtained and the method of harnessing this reaction to a useful work is to be stated.

Concept introduction:

The species that undergoes oxidation reaction loses electrons and thus gets oxidized. While the species that gains these electrons undergoes reduction process.

To determine: The reason of corrosion of most of the metals in air and the reason of difficulty in the corrosion of noble metals like gold, platinum, and silver.

Explanation

The balanced reaction for the given system is,

Mg(s)+2HCl(aq)MgCl2(aq)+H2(g)

When magnesium metal is added to a beaker of HCl(aq) , magnesium undergoes oxidation from zero to +2 oxidation state while hydrogen undergoes reduction from +1 to zero oxidation state. There is 1 chlorine atom on left hand side while there are 2 chlorine atoms on right hand side. Make them equal by multiplying HCl with a coefficient of 2

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