chemistry-class-11-unit-05-chapter-08-states-of-matter-gases-and-liquids-l-8-8-cdscprx6rzo

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Recap </primary>
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- $\text { Numerical examples }$
- $\text { Real gases }$
 - $\text { Van der Waals equation }$
 - $\text { Liquids } \left\\{\begin{array}{l}\text {vapor pressure} \\\ \text {surface tension} \\\ \text {viscosity}\end{array}\right.$

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<footer style = "font-size: 18px"> $\rightarrow$ States of matter gases and liquids $\rightarrow$ <span style = "color:blue"> Recap </span> $\rightarrow$ Experimental evidence for real gases $\rightarrow$ P-V graph </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Compressibility factor </primary>
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- $Z=\frac{pV}{nRT}$
- Z = 1 (at all pressures) shows ideal gas behaviour which is shown by $N_2, O_2, CO_2, CH_4$ gases
- At low pressure all gases behave ideally 
- Temperature at which Z= 1 for different gases is called boyle's temperature

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<footer style = "font-size: 18px"> $\rightarrow$ Continuity of liquid and gaseous states $\rightarrow$ <span style = "color:blue"> Compressibility factor </span> $\rightarrow$ Boyle's temeprature $\rightarrow$ Experimental observations </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Boyle's temeprature </primary>
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- Temperature at which Z= 1 for different gases is called boyle's temperature

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<footer style = "font-size: 18px">Continuity of liquid and gaseous states $\rightarrow$ Compressibility factor $\rightarrow$ <span style = "color:blue"> Boyle's temeprature </span> $\rightarrow$ Experimental observations $\rightarrow$ Pressure correction </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Pressure correction </primary>
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- Pressure of the gas arises from collision with the walls  
- $(\frac{n}{v})\times\frac{n}{v}$ $(\frac{n}{v})\rightarrow$
- First term shows correction in size of the molecule
- Second term shows correction in volume
- $P_{id} =(p+(\frac{n}{v})^2a)$

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<footer style = "font-size: 18px">Boyle's temeprature $\rightarrow$ Experimental observations $\rightarrow$ <span style = "color:blue"> Pressure correction </span> $\rightarrow$ Volume correction $\rightarrow$ Volume correction </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Volume correction </primary>
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- $V_{id} = (V - nb)$
- $P_{id} ~ V_{id} = nRT$
- $(p + (\frac{n}{v})^2a) (V - n b) = nRT$ 
- Van der Waals equation
- b- size of molecule
- a- intermolecular force

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<footer style = "font-size: 18px">Experimental observations $\rightarrow$ Pressure correction $\rightarrow$ <span style = "color:blue"> Volume correction </span> $\rightarrow$ Volume correction $\rightarrow$ Vander waal's equation </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Volume correction </primary>
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| $\text {Substance}$ | $a/bar L^2  mol^{-1}$ |$ b/L mol^{-1}$ |
| --------            | --------                        | --------         |
| $N_2$               |     $1.370$                     | $0.0387$         |
| $O_2$               |     $1.382$                     | $0.0319$         |
| $CO$                |     $1.472$                     | $0.0395$         |
| $CO_2$              |     $3.658$                     | $0.0429$         |
| $CH_4$              |     $2.303$                     | $0.0431$         |
| $C_2 H_6$           |     $5.580$                     | $0.0651$         |

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<footer style = "font-size: 18px">Pressure correction $\rightarrow$ Volume correction $\rightarrow$ <span style = "color:blue"> Volume correction </span> $\rightarrow$ Vander waal's equation $\rightarrow$ Things we have discussed </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Vander waal's equation </primary>
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- $\left(p+\frac{n^2 a}{v^2}\right)(v-n b)=n R T $

- $ \left(p+\left(\frac{n}{v}\right)^2 a\right)(v-n b)=n R T $

- $ p=\frac{n R T}{v-n b}-\left(\frac{n}{v}\right)^2 a$

- $\left(p+\frac{n^2 a}{v^2}\right)\rightarrow\text {cubic equation in V}$

- $\text {(a,b) different for different gases}$

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<footer style = "font-size: 18px">Volume correction $\rightarrow$ Volume correction $\rightarrow$ <span style = "color:blue"> Vander waal's equation </span> $\rightarrow$ Things we have discussed $\rightarrow$ Vapour pressure </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-8 </Success>
### <primary style="font-size:24px"> Surface tension </primary>
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- Spherical shape of small liquid drops
- Spheres - have the smallest surface area 
- Free surface energy 
- $\gamma A = \text { surface energy }$
- $\frac{d(\gamma A)}{d A}=\gamma +\frac{A d\gamma}{dA}  = 0 \text { for liquids }$
- $\gamma\rightarrow\frac{N}{m}\quad \gamma\rightarrow\text { surface tension }$

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<footer style = "font-size: 18px">Things we have discussed $\rightarrow$ Vapour pressure $\rightarrow$ <span style = "color:blue"> Surface tension </span> $\rightarrow$ Gasess law $\rightarrow$ Viscosity </footer>