Respuesta :
Complete the given reaction
[tex]$3 \mathrm{~N}_{2} \mathrm{O}(g)+6 \mathrm{H}^{+}(a q)+2 \mathrm{Cr}(s) \longrightarrow 3 \mathrm{~N}_{2}(g)+3 \mathrm{H}_{2} \mathrm{O}(l)+2 \mathrm{Cr}^{+3}(a q)$[/tex]
Write the oxidation reaction
[tex]$\mathrm{Cr}(s) \longrightarrow \mathrm{Cr}^{3+}(a q)+3 \mathrm{e}^{-} \quad E_{a d i}=+0.74 \mathrm{~V}$[/tex]
In the question the value of this reduction reaction is negative, but for oxidation reaction this sign is change as positive
Write the reduction reaction
[tex]$\begin{aligned}&\mathrm{N}_{2} \mathrm{O}(g)+2 \mathrm{H}^{+}(a q) 2 \mathrm{e}^{-} \longrightarrow \mathrm{N}_{2}(g)+\mathrm{H}_{2} \mathrm{O}(l) \\&E_{r e d}=+1.77 \mathrm{~V}\end{aligned}$[/tex]
Calculate the standard cell voltage
[tex]$E_{\text {ceU }}=E_{r e d}+E_{\text {oud }}$[/tex]
Substitute the value
[tex]$\begin{aligned}&E_{c e \bar{I}}=1.77+0.74 \\&E_{c e \overline{ }}=2.51 \mathrm{~V}\end{aligned}$[/tex]
Hence the standard cell potential is [tex]$2.51 \mathrm{~V}$[/tex]
Oxidizing agent in this reaction is
[tex]$\mathrm{N}_{2}(g), \mathrm{N}_{2} \mathrm{O}(g)$[/tex]
Reducing agent in this reaction is
[tex]$\mathrm{Cr}^{3+}(a q), \mathrm{Cr}(s)$[/tex]
A chemical process known as a reduction-oxidation or redox reaction happens when both reduction and oxidation take place simultaneously. While the oxidized species loses electrons, the reduced species gains them.
Reduction describes the increase in electrons. Oxidation and reduction always occur jointly because any loss of electrons by one substance must be followed by a gain of electrons by another. Therefore, oxidation-reduction processes or just redox reactions are other names for electron-transfer events.
Learn more about cell potential https://brainly.com/question/1313684
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