Question

Which of the following is true about the given redox reaction?
$SnC{l}_2+2FeC{l}_3\to SnC{l}_4+2FeC{l}_2$

• A. $SnC{l}_2$ is oxidised and $FeC{l}_3$ acts as oxidising agent.
• B. $FeC{l}_3$ is oxidised and acts as oxidising agent.
• C. $SnC{l}_2$ is reduced and acts as oxidising agent.
• D. $FeC{l}_3$ is oxidised and $SnC{l}_2$ acts as a oxidising agent.

Answer 1

Answer: (A)

$SnC{l}_2$ is oxidised and $FeC{l}_3$ acts as oxidising agent.

Separating the oxidation and reduction reaction from the redox reaction:

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

assigning the oxidation number on central atom ($Sn$ and $Fe$) in each molecules by considering oxidation number of $Cl=-1$ we get oxidation state as:

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

as the oxidation number of $Sn$ changes from +2 to +4 as:

$SnC{l}_2\to SnC{l}_4$

its a oxidation reaction where $SnC{l}_2$ gets oxidized and acts as reducing agent

Similarly, as the oxidation number of $Fe$ changes from +3 to +2 as:

$FeC{l}_3\to FeC{l}_2$

its a reduction reaction where $FeC{l}_3$ gets reduced and acts as oxidising agent.

Therefore $SnC{l}_2$ is oxidised and $FeC{l}_3$ acts as oxidising agent.