Chapter 19.2, Problem 16PP

Interpretation Introduction

Interpretation:

The given redox reaction is to be balanced using oxidation number method.

Concept introduction:

Oxidation number method involve:-

• Assign the oxidation number to each element.
• Check which element is oxidized and which element is reduced.
• Check the change in oxidation number for the elements which are oxidized and reduced.
• Balance the change in oxidation number by adjusting the coefficients in the equation.
• Then balance the other elements.

Answer to Problem 16PP

$3SnC{l}_4+2Fe\to 3SnC{l}_2+2FeC{l}_3$

Explanation of Solution

The given redox reaction is:

$SnC{l}_4+Fe\to SnC{l}_2+FeC{l}_3$

Assigning the oxidation number-

$\stackrel{+4}{Sn}\stackrel{-1}{C{l}_4}+\stackrel{0}{Fe}\to \stackrel{+2}{Sn}{\stackrel{-1}{Cl}}_2+\stackrel{+3}{Fe}\stackrel{-1}{C{l}_3}$

The oxidation numbers of atoms shows that

$Fe$ is oxidized and $Sn$ is reduced.

Change in oxidation number of $Fe=+3$

Change in oxidation number of $Sn=-2$

Thus adjusting the coefficients:

$3SnC{l}_4+2Fe\to 3SnC{l}_2+2FeC{l}_3$

Conclusion

Thus the balanced redox equation is:

$3SnC{l}_4+2Fe\to 3SnC{l}_2+2FeC{l}_3$