chemistry-class-11-unit-05-chapter-05-states-of-matter-gases-and-liquids-l-5-8-20h9cethy2u

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Three gas laws </primary>
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- $\text {Boyle's law}$
- $P \propto \frac{1}{V} / V \propto \frac{1}{P}$
- $P V= \text {constant}$
- $\text {Charles or Gay-Lussac}$
- $V \propto T$
- $\text {Avogadro's hypothesis}$
- $V \propto \mathrm {n}$
- $\text {Gay-Lussac (combining volumes)}$

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<footer style = "font-size: 18px">STATES OF MATTER $\rightarrow$ States of matter $\rightarrow$ <span style = "color:blue"> Three gas laws </span> $\rightarrow$ Introduce Ideal gas equation $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Introduce Ideal gas equation </primary>
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- Relate mass, pressure , volume , temperature to individual molecules in a gas
- Avogadro's hypothesis
- Dalton proposed that each atom is same as every other atom in a sample - atomic mass
- Mass of sample = Nm
	
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<footer style = "font-size: 18px">States of matter $\rightarrow$ Three gas laws $\rightarrow$ <span style = "color:blue"> Introduce Ideal gas equation </span> $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Kinetic molecular model for gases(kinetic's theory) </primary>
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- Gases occupy space and are made up of  molecules
- The mass of the gas is due to molecules- molecules lead to the mass
- Molecules occupy no volume 
- Dalton - all molecules have the same mass

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<footer style = "font-size: 18px">Introduce Ideal gas equation $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ <span style = "color:blue"> Kinetic molecular model for gases(kinetic's theory) </span> $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Kinetic molecular model for gases(kinetic's theory) </primary>
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- Molecules are in ceaseless random motion 
- Molecules move in straight lines - undergo collisions with other molecules or with the walls of the container

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<footer style = "font-size: 18px">Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ <span style = "color:blue"> Kinetic molecular model for gases(kinetic's theory) </span> $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Kinetic molecular model for gases(kinetic's theory) </primary>
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- The motion is random with respect to the rate and direction
 - Speeds - zero to very high values 
 - Direction - random 
- Kinetic energy varies with times at any temperature the average kinetic energy per molecules in the same for all molecules in all gases - temperature is proportional to kinetic energy

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### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Kinetic molecular model for gases(kinetic's theory) </primary>
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- Conservation of energy   $\frac{1}{2} mv^2$
- $\frac{1}{2} m v_{black}^2 \neq \frac{1}{2} mv^2_{\text{blue}}$= constant
- Elastic collision
- $\langle K E\rangle = \frac{1}{2}m\frac{v_{black}^2+v_{blue}^2+v_{green}^2+v_{red}^2}{4}$
- $\langle K E\rangle = \overrightarrow{KE}$

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<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/bc85fccf-c6e6-43ed-0b00-e045be0b3d00/public" width="80%">
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<footer style = "font-size: 18px">Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ <span style = "color:blue"> Kinetic molecular model for gases(kinetic's theory) </span> $\rightarrow$ Motion of molecules $\rightarrow$ Kinetic theory of gases </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Motion of molecules </primary>
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- Conservation of momentum
 - $m_1 \vec {v_1} + m_2 \vec {v_2} = \text {constant}$
 - Kinetic theory of gases

| Molecules                      | Motion                     | Avogadro hypothesis |
| --------                       | --------                   | --------            |
|1. Mass in molecules            |1. Random rate and direction|                     |
|2. Zero volume of molecules     |2. Straight  lines          |                     |
|3. Molecules with identical mass|3. KE $\propto$ T           |                     |
|                                |4. Conservation of energy   |                     |
|                                |5. Momentum                 |                     |

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<footer style = "font-size: 18px">Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ <span style = "color:blue"> Motion of molecules </span> $\rightarrow$ Kinetic theory of gases $\rightarrow$ Kinetic energy of gas molecules </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Kinetic theory of gases </primary>
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- Absolute zero
 - Volume arises as a result of motion 
 - v = 0 $\Rightarrow$ no motion 
 - v $\geqslant 0$ , motion $\geqslant 0$
 - absolute zero $\rightarrow$ no motion 
- Kinetic energy is zero
 - $T(^oC) $ $\rightarrow T (K)$
  - $273.15 + \mathrm {T}(^o\mathrm {C})  = \mathrm {T}(\mathrm {K})$
	
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<footer style = "font-size: 18px">Kinetic molecular model for gases(kinetic's theory) $\rightarrow$ Motion of molecules $\rightarrow$ <span style = "color:blue"> Kinetic theory of gases </span> $\rightarrow$ Kinetic energy of gas molecules $\rightarrow$ Kinetic energy of gas molecules </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Kinetic energy of gas molecules </primary>
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- **Two samples of two  different gases**
- One sample has mass $m_1$ in $N_1$ container
- Other sample has mass $m_1$ in $N_1$ container
- $(m_1)N_1$ identical containers  $(m_2) N_2$
- Avogadro convers $\rightarrow$ pressure is the same 
- $\frac{1}{2} m_1 ~ v_1^2=\frac{1}{2} m_2 ~ v_2^2$
- $\frac{v_1^2}{v_2^2}=\frac{m_2}{m_1} $
- $\frac{v_1}{v_2}=\sqrt{\frac{m_2}{m_1}}$

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<footer style = "font-size: 18px">Motion of molecules $\rightarrow$ Kinetic theory of gases $\rightarrow$ <span style = "color:blue"> Kinetic energy of gas molecules </span> $\rightarrow$ Kinetic energy of gas molecules $\rightarrow$ Graham's law of effusion </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Kinetic energy of gas molecules </primary>
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- $\frac{1}{2} m_1 \bar{~ v}_1 ^2 = \frac{1}{2} m_2 \bar{~ v}_2 ^2$
- $\bar{~ v}_1 ^2$ = Average velocity
- $\frac{\bar{v_1}}{\bar{v_2}} = \sqrt{\frac{m_2}{m_1}}$
- $\frac{\bar{v_1}}{\bar{v_2}}=\frac{\text{collision frequency in 1/area}}{\text{collision frequency in 2/area}}$
- $\frac{\sqrt{m_2}}{\sqrt{m_1}}$

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<footer style = "font-size: 18px">Kinetic theory of gases $\rightarrow$ Kinetic energy of gas molecules $\rightarrow$ <span style = "color:blue"> Kinetic energy of gas molecules </span> $\rightarrow$ Graham's law of effusion $\rightarrow$ Temperature and pressure </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-5 </Success>
### <primary style="font-size:24px"> Temperature and pressure </primary>
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- $V \propto \frac{1}{P}$ (Boyle) at constant T and number of molecules
- $V \propto T$ (Gay - Lussac or charles)
- $V \propto n$
- $PV = nRT$
- n = number of moles
- R = universal gas constant
- T = temperature in kelvin
- V = volume
- P = pressure
- Ideal gas equation of state

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<footer style = "font-size: 18px">Graham's law of effusion $\rightarrow$ Temperature and pressure $\rightarrow$ <span style = "color:blue"> Temperature and pressure </span> $\rightarrow$ Thank you $\rightarrow$  </footer>