Respuesta :
E°cell for each reaction, and rank the strengths of the oxidizing and reducing agents:
Complete the given reaction
[tex]$3 \mathrm{Au}^{+}(a q)+\mathrm{Cr}(s) \longrightarrow 3 \mathrm{Au}(s)+\mathrm{Cr}^{+3}(a q)$[/tex]
Write the oxidation reaction
[tex]$\mathrm{Cr}(s) \longrightarrow \mathrm{Cr}^{3+}(a q)+3 \mathrm{e}^{-}$[/tex]
[tex]$E_{a x d}=+0.74 \mathrm{~V}$[/tex]
Write the reduction reaction
[tex]$\mathrm{Au}^{+}(a q)+e^{-} \longrightarrow \mathrm{Au}(s)$[/tex]
[tex]$E_{r e d}=+1.69 \mathrm{~V}$[/tex]
Calculate the standard cell voltage
[tex]$E_{c ell}=E_{r e d}+E_{c u d}$[/tex]
Substitute the value
[tex]$\begin{aligned}&E_{cell}=1.69+0.74 \\&E_{c e \mathbb{I}}=2.43 \mathrm{~V}\end{aligned}$[/tex]
Hence the standard cell potential is [tex]$2.43 \mathrm{~V}$[/tex]
The oxidizing agent in this reaction is
[tex]$\mathrm{Au}^{+}(a q), \mathrm{Au}(s)$[/tex]
Reducing agent in this reaction is
[tex]$\mathrm{Cr}^{3+}(a q), \mathrm{Cr}(s)$[/tex]
A chemical process known as an oxidation-reduction (redox) reaction includes the exchange of electrons between two substances. Any chemical reaction in which the oxidation number of a molecule, atom, or ion changes due to the gain or loss of an electron is referred to as an oxidation-reduction reaction.
Redox reactions include a change in the oxidation state of the substrate. Loss of electrons or a rise in an element's oxidation state are both considered to be oxidation. Gaining electrons or lowering the oxidation state of an element or its constituent atoms are both examples of reduction.
Learn more about oxidation reaction https://brainly.com/question/19528268
#SPJ4
