chemistry-class-11-unit-05-chapter-06-states-of-matter-gases-and-liquids-l-6-8-tykzvmuenhu

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Kinetic theory of gases </primary>
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- Molecules (all mass , zero volume)
- Motion of molecules (straight line , rate and direction is random KE $\propto$ T , average KE is same for all molecules , conservation of energy and momentum during collision)
- Avogadro's postulate

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<footer style = "font-size: 18px"> $\rightarrow$ States of matter $\rightarrow$ <span style = "color:blue"> Kinetic theory of gases </span> $\rightarrow$ Gaseous law $\rightarrow$ Gaseous law </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Gaseous law </primary>
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- Pressure - arises as a result of collision with the walls of the container
- $ V \propto \frac{1}{P}$ ( at constant T and for fixed mass)
- $ PV = K \quad K= kT$
- $PV = kT - \text {Boyle's law}$
- At constant pressure
- $ V = \frac{kT}{P} \quad V \propto T \text{(Gay-Lussac's law)}$

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<footer style = "font-size: 18px">States of matter $\rightarrow$ Kinetic theory of gases $\rightarrow$ <span style = "color:blue"> Gaseous law </span> $\rightarrow$ Gaseous law $\rightarrow$ Gaseous law </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Gaseous law </primary>
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- $\mathrm {PV = kT}$
- At fixed volume 
- $P=\frac{kT}{V}$
- $P\propto T$ (Gay-Lussac)
- $\mathrm {PV = kT} \rightarrow $Assumption that are in kenetic theroy of gasses
- Product $PV \propto T$
- PV = kT
- $\frac{\text{Force}}{\text{area}}\times \text{ area} \times\text{ length} $
- PV units of energy

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<footer style = "font-size: 18px">Kinetic theory of gases $\rightarrow$ Gaseous law $\rightarrow$ <span style = "color:blue"> Gaseous law </span> $\rightarrow$ Gaseous law $\rightarrow$ Helium gas (PV-T variation ) </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Helium gas (PV-T variation ) </primary>
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- Helium at $0^{\circ} \mathrm{C}$ 273.15K occupies 1 liter at 1 atm $\rightarrow$ vary T, PV product

| $T / K$                 | $T^o \mathrm {c} $ | $\text {PV/l-atm}$ |
| --------                | --------           | --------           |
|273.15= 373.15   |$100^o\mathrm{c}$   |$1.359$             |
|                      |$50^o\mathrm{c} $   |$1.1830$            |
|                        |$0^{\circ}$         |$1.00$              |
|                       |$-50^{\circ} $      |$0.8171$            |
|                        |$-100^{\circ}$      |$0.6341$            |

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<footer style = "font-size: 18px">Gaseous law $\rightarrow$ Gaseous law $\rightarrow$ <span style = "color:blue"> Helium gas (PV-T variation ) </span> $\rightarrow$ Helium gas (PV-T variation ) $\rightarrow$ Helium gas (PV-T variation ) </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Helium gas (PV-T variation ) </primary>
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- Gay - Lussac
- $V\propto T$
- $\text {Slope}=\frac{Rise}{run}$
- $PV\propto T$

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<footer style = "font-size: 18px">Gaseous law $\rightarrow$ Helium gas (PV-T variation ) $\rightarrow$ <span style = "color:blue"> Helium gas (PV-T variation ) </span> $\rightarrow$ Helium gas (PV-T variation ) $\rightarrow$ Molar Volume of gases </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Helium gas (PV-T variation ) </primary>
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- Helium 
- Volume occupied by 1 mole of helium at $0{ } ^oC(273 K)$ and 1 atm pressure $\rightarrow$ molar volume
- Density = $\frac{\text{mass}}{\text{volume}}$
- Molecular mass = 4.00 g/mol
- Volume = $\frac{4.0039}{0.1785 g/L}$
- 22.43 L
- Avogadro number of molecule
- Molar volume = 22.43L

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<footer style = "font-size: 18px">Helium gas (PV-T variation ) $\rightarrow$ Helium gas (PV-T variation ) $\rightarrow$ <span style = "color:blue"> Helium gas (PV-T variation ) </span> $\rightarrow$ Molar Volume of gases $\rightarrow$ Molecular nature of ideal gas </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Molar Volume of gases </primary>
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- All gases should occupy 22.4L at $0^{\circ}c $ and 1 atm pressure

|           | $\text {electrons}$ | $\text {molar volume} \mathrm {~ L ~ mol} ^{-1}$ |
| --------  | --------            | --------                                         |
| $He$      |2                    | 22.415                                           |
| $H_2 $    |2                    | 22.428                                           |
| $ NH_3$   |10                   | 22.077                                           | 
| $CH_4 $   |10                   | 22.360                                           |
| $Ne$      |10                   | 22.428                                           |

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<footer style = "font-size: 18px">Helium gas (PV-T variation ) $\rightarrow$ Helium gas (PV-T variation ) $\rightarrow$ <span style = "color:blue"> Molar Volume of gases </span> $\rightarrow$ Molecular nature of ideal gas $\rightarrow$ Value of k </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Molecular nature of ideal gas </primary>
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- Mass of gas due to molecules 
- Volume of gas is space between molecules 
- Molecules are in motion at all $\mathrm {T > 0k}$ in straight lines 
- Move at random 
- Average $KE \propto T$
- When molecules collide , conserve energy and momentum
- At any temperature equal volumes of all gases contain equal number of  molecule

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<footer style = "font-size: 18px">Helium gas (PV-T variation ) $\rightarrow$ Molar Volume of gases $\rightarrow$ <span style = "color:blue"> Molecular nature of ideal gas </span> $\rightarrow$ Value of k $\rightarrow$ Ideal gas equation </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Value of k </primary>
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- PV = kT
- 1 mol of helium , molar volume = 22.4 L
- P = 1 atm at 273K
- $k = \frac{1 \operatorname{atm} \times 22.4 \mathrm{L} / \mathrm{mol}}{273 \mathrm{K}}$
- 0.082 L atm / k / mol
- 8.314 J / K /mol
- k = function of P , V , T
- For 2 moles
- k = 0.164  L atm/K

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<footer style = "font-size: 18px">Molar Volume of gases $\rightarrow$ Molecular nature of ideal gas $\rightarrow$ <span style = "color:blue"> Value of k </span> $\rightarrow$ Ideal gas equation $\rightarrow$ Validity of kinetic theory </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-6 </Success>
### <primary style="font-size:24px"> Ideal gas equation and Dalton's law </primary>
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- $P V=n R T$
- Ideal gas equation of state
- Dalton's law PV = $(n_1+n_2+n_3+\cdots)$ RT
- Mixture of many gases
- Dalton's law
- $P  =\frac{1}{v}\left(n_1+n_2+n_3+\cdots\right)$ RT
- $\frac{n_1 R T}{v}+\frac{n_2 R T}{v}+\frac{n_3 R T}{v}+\cdots$
- $P_1 +P_2+P_3+\cdots$
- $n_i = \frac{x_i}{n}$
- $ {x_i}\rightarrow\text{mole fraction}$

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<footer style = "font-size: 18px">Ideal gas equation $\rightarrow$ Validity of kinetic theory $\rightarrow$ <span style = "color:blue"> Ideal gas equation and Dalton's law </span> $\rightarrow$ Numerical examples $\rightarrow$ Numerical examples </footer>