chemistry-class-11-unit-08-chapter-02-redox-reactions-l-2-3-uyxofkl-v4o

### <Success style="font-size:25px"> Redox Reactions L-2 </Success>
### <primary style="font-size:24px"> Redox reaction </primary>
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- Electron transfer reaction

- $H_2O \rightarrow O_2 $

- Glucose $\rightarrow$ ATP

- Glucose $\rightarrow CO_2+H_2O$

- $E^o$, $\Delta G$, $\Delta H$

- $\Delta H$- exothemic endothermic experiments

- $A+O_2 \rightarrow AO or AO_2$- combination reaction

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<footer style = "font-size: 18px"> $\rightarrow$ Redox reaction $\rightarrow$ <span style = "color:blue"> Redox reaction </span> $\rightarrow$ Redox reaction $\rightarrow$ Redox reaction </footer>

### <Success style="font-size:25px"> Redox Reactions L-2 </Success>
### <primary style="font-size:24px"> Redox reaction </primary>
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* Two half reactions (at pH-0)

* Oxidation $2H_2O \rightarrow 4H^++4e^-+O_2$ $\hspace{2mm}$ $E^o$= 1.23 V vs NHE

* Reduction $4H^+4e^- \rightarrow 2H_2$ $\hspace{2mm}$ $E^o$ = 0.00 V vs NHE

* Overall $2H_2O \rightarrow 2H_2+O_2$ $\hspace{2mm}$ $E^o cell$ = 1.23 V, $\Delta G$ -475 kJ/mol

* **Water as an oxidant-** Reaction of Na (having negative standard potential) metal with water release $H_2$ from water

- $Na+H_2O \rightarrow Na^++HO^-+ \frac{1}{2} H_2$ - water serving as oxidant

* **Water as a reductant-**

- $2H_2O+2F_2 \rightarrow 4F+4H^++O_2$ - oxidation of water

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<footer style = "font-size: 18px">Redox reaction $\rightarrow$ Redox reaction $\rightarrow$ <span style = "color:blue"> Redox reaction </span> $\rightarrow$ Redox reaction $\rightarrow$ Oxidisation and reduction </footer>

### <Success style="font-size:25px"> Redox Reactions L-2 </Success>
### <primary style="font-size:24px"> Redox reaction </primary>
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* Some oxides, especially of weakly electro +ve metals decompose when heated to high enough temperature a classical example is the decomposition of $\mathrm{HgO}$ to give oxygen and $\mathrm{Hg}$

* The more reactive metal displaces the less reactive metal from its oxide also

\mathrm{Zn}+\mathrm{CuO} \rightarrow \mathrm{ZnO}+\mathrm{Cu}$$

* Extraction of these elements requires redox chemistry using appropriate reducing and oxidizing agenst

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<footer style = "font-size: 18px">Redox reaction $\rightarrow$ Redox reaction $\rightarrow$ <span style = "color:blue"> Redox reaction </span> $\rightarrow$ Oxidisation and reduction $\rightarrow$ Metallurgy </footer>

### <Success style="font-size:25px"> Redox Reactions L-2 </Success>
### <primary style="font-size:24px"> Oxidisation and reduction </primary>
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* Iron is produced in greater quantities than any other metal by reduction of $\mathrm{F}_2 \mathrm{O}_3$ with carbon (coke)

* Carbon reduction also for $-\mathrm{Si}, \mathrm{P}, \mathrm{Mn}$ and $\mathrm{Sn}$

- $2 \mathrm{Fe}_2 \mathrm{O}_3+3 \mathrm{C} \rightarrow 4 \mathrm{Fe}+3 \mathrm{CO}_2$

* At $25^{\circ} \mathrm{C}, \Delta \mathrm{G}^{\circ}$ is $+151 \mathrm{kJ} \mathrm{mol}^{-1}$
- Not a thermodynamically feasible reaction at RT Blast furnace above $100{ }^{\circ} \mathrm{C}$

* For highly electro +ve metals like $\mathrm{Ca}, \mathrm{Al}, \mathrm{Mg}$ the oxides are too stable ( $\Delta \mathrm{G}^{\circ}$ is too negative) - thus reqd temperature would be very high
- $\mathrm{Al}$ is extracted from molten $\mathrm{Al}_2 \mathrm{O}_3$

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<footer style = "font-size: 18px">Redox reaction $\rightarrow$ Redox reaction $\rightarrow$ <span style = "color:blue"> Oxidisation and reduction </span> $\rightarrow$ Metallurgy $\rightarrow$ Reactions </footer>

### <Success style="font-size:25px"> Redox Reactions L-2 </Success>
### <primary style="font-size:24px"> Metallurgy </primary>
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* Fe $\rightarrow$ $Fe_2O_3$ (Ore/Rust )

* $Al +O_2 \rightarrow Al_2O_3$

* $Mg+O_2 \rightarrow MgO$

* $Ba+F_2 \rightarrow BaF_2$

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<footer style = "font-size: 18px">Redox reaction $\rightarrow$ Oxidisation and reduction $\rightarrow$ <span style = "color:blue"> Metallurgy </span> $\rightarrow$ Reactions $\rightarrow$ Decomposition reactions </footer>

### <Success style="font-size:25px"> Redox Reactions L-2 </Success>
### <primary style="font-size:24px"> Decomposition reactions </primary>
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* Ca-oxalate $\rightarrow CaCO_3 \rightarrow CaO+CO_2$

* $NaH \xrightarrow {\Delta} Na^0 + H_2^0$

* $LiAlH_4$ and $NaBH_4$ are the redusing agent

* $2KClO_3 \rightarrow 2KCl+3O_2$

* Thermal stability of $NH_4NO_2$ and $NH_4NO_3$ is very less

* $NH_4NO_2 \xrightarrow {\Delta} N_2 + 2H_2O$

* $NH_4NO_3 \xrightarrow {\Delta} N_2O + 2H_2O$

* The oxidising power increas as $Cl^- < NO_2^{-} < NO_3^{-}$

* $(NH_4)_2 Cr_2O_7 \xrightarrow {\Delta} N_2 + Cr_2O_3 + 4H_2O$

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<footer style = "font-size: 18px">Metallurgy $\rightarrow$ Reactions $\rightarrow$ <span style = "color:blue"> Decomposition reactions </span> $\rightarrow$ Thank you $\rightarrow$  </footer>