chemistry-class-11-unit-07-chapter-03-chemical-equillibrium-l-3-8-yzs48rqplha

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Equilibrium constant </primary>
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* $aA + bB \rightleftharpoons cC+dD$

* K = $\frac{[C]^c[D]^d}{[A]^a[B]^b}$

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<footer style = "font-size: 18px"> $\rightarrow$ Chemical equilibrium $\rightarrow$ <span style = "color:blue"> Equilibrium constant </span> $\rightarrow$ Importance of K $\rightarrow$ Value of equilibrium constant </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Value of equilibrium constant </primary>
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- Consider two reactions

* $CoO (s) + H_2(g) \rightleftharpoons CoO (s) + H_2 O (g) \rightarrow K_1$ -(i)

* $CoO (s) + CO (g) \rightleftharpoons Co (s) + CO_2 (g) \rightarrow K_2$ - (ii)

* $CO_2 (g) + H_2 (g) \rightleftharpoons CO(g) + H_2O (g) \rightarrow K$ - (iii)

* $K$ can be expressed in terms of $K_1$ and $K_2$

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<footer style = "font-size: 18px">Equilibrium constant $\rightarrow$ Importance of K $\rightarrow$ <span style = "color:blue"> Value of equilibrium constant </span> $\rightarrow$ Value of equilibrium constant $\rightarrow$ Value of equilibrium constant </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Value of equilibrium constant </primary>
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* $CoO (s) + H_2(g) \rightleftharpoons Co (s) + H_2O (g)$ - (i)

* $CoO (s) + CO (g) \rightleftharpoons Co (s) + CO_2 (g) $ - (ii)

* $k_1 =\frac{H_2O(g)}{H_2 (g)} , K_2 =\frac{CO_2(g)}{CO(g)}$

* $CO_2(g) + H_2 (g) \rightleftharpoons CO(g) + H_2O (g)$

* $K=\frac{\left(\mathrm{CO}(g)\left(\mathrm{H}_2O (q)\right)\right.}{H_2(g)(\mathrm{CO}_2)(g)}=\frac{K_1}{K_2}$

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<footer style = "font-size: 18px">Importance of K $\rightarrow$ Value of equilibrium constant $\rightarrow$ <span style = "color:blue"> Value of equilibrium constant </span> $\rightarrow$ Value of equilibrium constant $\rightarrow$ Value of equilibrium constant </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Value of equilibrium constant </primary>
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* $2SO_2(g) + O_2(g) \rightleftharpoons 2SO_3(g)$

* $K_p$ is known

* $2SO_3(g)  \xtofrom[{K_p^{'}}]{} 2SO_2(g) + O_2(g)$

* $K_p^{'}$ $=\frac{(P_{SO_2})^{2}(P_{O_2})}{(P_{SO_3})^2}$ = $\frac{(1/P_{SO_3})^2}{(P_{SO_2})^{2}(P{O_2})}$ 
* $K_p^{'} =\frac{1}{K_p}$

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<footer style = "font-size: 18px">Value of equilibrium constant $\rightarrow$ Value of equilibrium constant $\rightarrow$ <span style = "color:blue"> Value of equilibrium constant </span> $\rightarrow$ Value of equilibrium constant $\rightarrow$ Value of equilibrium constant </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Value of equilibrium constant </primary>
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* $2SO_2 (g) + O_2(g) \rightleftharpoons 2SO_3(g)$

* $K_p$ is known

* $SO_2(g) + \frac{1}{2} O_2(g)  \xtofrom[{K_p^{'}}]{} S_3(g)$

* $K_p^{'} =\frac{(P_{SO_3})}{(P_{SO_2})(g)(P_{O_2})^{1/2}}$

* $K_p^{'}$=$\sqrt{\frac{(P_{SO_3})^2}{P_{SO_2}^2 P_{O_2}}}$ = $K_p^ {1/2}$

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### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Value of equilibrium constant </primary>
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* A + B $\rightleftharpoons$ C + D $\quad$ $K_1$

* C + D $\rightleftharpoons$ A + B $\quad$ $K_2$

* $K_1 = \frac{1}{K_2}$

* A + B $\rightleftharpoons$ C + D $\quad$ $K_1$

* $\frac{1}{2}A + \frac{1}{2} B \rightleftharpoons \frac{1}{2}C+\frac{1}{2}D K_1^{'}$

* $K_1^{'} =(K_1)^{1/2}$

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### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Le Chatelier's priniciple </primary>
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* Effect of pressure

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<footer style = "font-size: 18px">Le Chatelier's priniciple $\rightarrow$ Le Chatelier's priniciple $\rightarrow$ <span style = "color:blue"> Le Chatelier's priniciple </span> $\rightarrow$ Effect of pressure $\rightarrow$ Effect of pressure </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Effect of pressure </primary>
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* $2SO_2 (g) + O_2(g)$ $\rightleftharpoons$ $2SO_3 (g)$

* $K_P = K_x\times (P)^{2-(2+1)}$

- $ K_x \times (P)^{-1} =\frac{K_x}{P}$

- If there is increase in the pressure ,then there should be increase in $K_x$ so that the $K_P$ remains constant

- This means forward reaction will be favoured

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<footer style = "font-size: 18px">Le Chatelier's priniciple $\rightarrow$ Effect of pressure $\rightarrow$ <span style = "color:blue"> Effect of pressure </span> $\rightarrow$ Effect of pressure $\rightarrow$ Change in pressure </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Change in pressure </primary>
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* Pressure can be changed by introduction of inert gas

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<footer style = "font-size: 18px">Effect of pressure $\rightarrow$ Effect of pressure $\rightarrow$ <span style = "color:blue"> Change in pressure </span> $\rightarrow$ Change in pressure $\rightarrow$ Effect of inert gas on equilibrium </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Change in pressure </primary>
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* $PCl_5 (g) \rightleftharpoons PCl_3 (g) +Cl_2 (g)$

* $K_p = \frac{(P_{PCl_3})(P_{Cl_2})}{(P_{PCl_5})}$

* $K_p = \frac{(x_{PCl_3}\times P)}{(x_{Cl_2}\times P)}$

* $K_p = \frac{\frac{n_{PCl_3}}{\Sigma_n} \times \frac{n_{Cl_2}}{\Sigma_n}}{(n_{PCl_5}/\Sigma_n)}$ $\times P$

* $K_p = \frac{n_{PCl_3}n_{Cl_2}\times P}{n_{PCl_5}\times\Sigma n}$

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<footer style = "font-size: 18px">Effect of pressure $\rightarrow$ Change in pressure $\rightarrow$ <span style = "color:blue"> Change in pressure </span> $\rightarrow$ Effect of inert gas on equilibrium $\rightarrow$ Effect of increase in pressure </footer>

### <Success style="font-size:25px"> Chemical Equilibrium L-3 </Success>
### <primary style="font-size:24px"> Effect of inert gas on equilibrium </primary>
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* $PCl_5 (g) \rightarrow PCl_3 (g) + Cl_2 (g)$

* $K_p=\frac{P_{PCl_3} P_{Cl_2}}{P_{PCl_5}}$

* $K_p=\frac{n_{PCl_3}}{\Sigma_n}\times \frac{n_{Cl_2}}{\Sigma_n}\times P^2 / \frac{n_{PCl_5}}{\Sigma_n} \times P$

* $K_p=\frac{n_{PCl_3}\times n_{Cl_2}}{n_{PCl_5} \times \Sigma_n} \times P$
* if $\Sigma_n$ increase, forward reaction will be favoured
* if $\Sigma_n$ decrease, reverse reaction will be favoured

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<footer style = "font-size: 18px">Change in pressure $\rightarrow$ Change in pressure $\rightarrow$ <span style = "color:blue"> Effect of inert gas on equilibrium </span> $\rightarrow$ Effect of increase in pressure $\rightarrow$ Thank you </footer>