chemistry-class-11-unit-05-chapter-04-states-of-matter-gases-and-liquids-l-4-8-7k-sszizubw

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Robert Boyle's experiment </primary>
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| Number of spaces in the short leg of the manometer tube |(h) Height different between the two Hg level | h+29.1 inches |
| --------                                                 | --------                                     | --------      |
| 48                                                       | 0.0                                          | 29.1 inches   |

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![image](https://temp-public-img-folder.s3.ap-south-1.amazonaws.com/sathee.prutor.images/subject-images/iitpal/image/chemistry-class-11-unit-05-chapter-04-states-of-matter-gases-and-liquids-l-4_8-7k-sszizubw-138-0655.2.jpg)

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<footer style = "font-size: 18px">Robert Boyle's experiment $\rightarrow$ Robert Boyle's experiment $\rightarrow$ <span style = "color:blue"> Robert Boyle's experiment </span> $\rightarrow$ Mercury manometer $\rightarrow$ Mercury manometer </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Mercury manometer </primary>
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| Number of spaces in the short leg of the manometer tube |Height different between the two Hg level | h+29.1 inches |
| --------                                                 | --------                                 | --------      |
| 48                                                       | 0.0                                      |29.1 in        |
| 44                                                       | 2.8                                      |31.9 in        |
| 40                                                       | 6.2                                      |35.3           |
| 36                                                       | 10.1                                     |39.2           |
| 32                                                       | 15.1                                     |44.2           |
| 28                                                       | 21.2                                     |50.3           |

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<img src="https://imagedelivery.net/YfdZ0yYuJi8R0IouXWrMsA/9cacb343-0faf-485d-6a2b-e025c64a2600/public" width="80%">
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<footer style = "font-size: 18px">Robert Boyle's experiment $\rightarrow$ Robert Boyle's experiment $\rightarrow$ <span style = "color:blue"> Mercury manometer </span> $\rightarrow$ Mercury manometer $\rightarrow$ V versus graph </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Charles law </primary>
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- $\Delta V \propto \Delta T (\text {Charles Law})$
- $\Delta V=k' \Delta T$
- $\frac{V_2}{V_1} \frac{\text { at } 100^{\circ} {C}}{\text { at } 0^{\circ}{C}} =1.375$
- This is independent of gas
- For a fixed amount of gas this ratioworks out to be 1.366

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<footer style = "font-size: 18px">V versus graph $\rightarrow$ Volume on temperature $\rightarrow$ <span style = "color:blue"> Charles law </span> $\rightarrow$ Plot of volume versus temperature $\rightarrow$ Units of volume </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Units of volume </primary>
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- $ \mathrm {SI} \rightarrow \mathrm {m^3}$
- $ \mathrm {dm}^3 / 1 \mathrm {dm}=0.1 {\mathrm {m}}$
- $ 1 \mathrm {dm}^3=10^{-3}\mathrm {m}^3 $
- $ \text { Liter } \equiv 1000 \mathrm {cm}^3 $
- $ 100 \mathrm {cm} \equiv 1 {m} $
- $ \mathrm {mL} \equiv 10^{-3}{L}$

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<footer style = "font-size: 18px">Charles law $\rightarrow$ Plot of volume versus temperature $\rightarrow$ <span style = "color:blue"> Units of volume </span> $\rightarrow$ Units of pressure $\rightarrow$ Units of pressure </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Units of pressure </primary>
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- 1 Atmosphere = 760 mm of Hg
- Pascal(Pa) = SI unit of pressure
- $P = \frac{F}{A} = \frac{m\times a}{area} = \frac{\mathrm {kg ms}^{-2}}{~ m^2}$
- $ 10^5 \mathrm{~Pa} = 1 \text { bar }$
- mm  of  Hg $\rightarrow$ atmosphere $\rightarrow$ Pa $\rightarrow$  bar

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<footer style = "font-size: 18px">Units of volume $\rightarrow$ Units of pressure $\rightarrow$ <span style = "color:blue"> Units of pressure </span> $\rightarrow$ Boyle's law $\rightarrow$ Boyle's law </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Boyle's law </primary>
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- **Relationship between pressure  to volume**
- $\mathrm {1.53 ~ L ~ of ~ SO_2}$ gas at a pressure of $5.6 \times 10^3 \mathrm {Pa}$ pressure in changed to $1.5\times10^4 \mathrm {Pa}$. what is the volume occupied by $\mathrm {SO_2}$ gas under the new condition ?

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<footer style = "font-size: 18px">Units of pressure $\rightarrow$ Units of pressure $\rightarrow$ <span style = "color:blue"> Boyle's law </span> $\rightarrow$ Boyle's law $\rightarrow$ Example of Charles law </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Boyle's law </primary>
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- **Solution**
- $P_1=5.6 \times 10^3{Pa} \quad V_1 = 1.53 {L}$
- $ P_2=1.5 \times 10^4 {Pa} \quad V_2 = \text { ? }$
- $P \propto \frac{1}{V}\quad \text { or }\quad V \propto \frac{1}{P}$
- $ P_1 V_1 = P_2 ~ V_2 \quad \frac{P_2}{P_1} = \frac{V_1}{V_2}$
- $V_2=\frac{P_1 V_1}{P_2}$

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<footer style = "font-size: 18px">Units of pressure $\rightarrow$ Boyle's law $\rightarrow$ <span style = "color:blue"> Boyle's law </span> $\rightarrow$ Example of Charles law $\rightarrow$ Example of charles law </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-4 </Success>
### <primary style="font-size:24px"> Example of Charles law </primary>
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- $A$ sample of gas at $15 ^o\mathrm {C}$ and 1 atmospheric pressure has a volume of $2.58 {L}$ what volume will this gas occupy at $38^o\mathrm {C}$ and 1 atmospheric ?

- **Solution**
- $T_1$ = (273.15+15)K
- $T_2$ = (273.15+38)K
- $V_1$ = 2.58 {L}
- V $\propto$ T
- $  \frac{V_1}{T_1} = \frac{V_2}{T_2}$
- $\frac{2.58 L}{288.15 {K}} = \frac{V_2(L)}{311.15K}$

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<footer style = "font-size: 18px">Boyle's law $\rightarrow$ Boyle's law $\rightarrow$ <span style = "color:blue"> Example of Charles law </span> $\rightarrow$ Example of charles law $\rightarrow$ Avogadro's hypothesis </footer>

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### <primary style="font-size:24px"> Practical use </primary>
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- $\text {Cars} \rightarrow \text {air bags}$
- Air bags of volume 36L with $N_2$ gas at 1.15 atm and $26^o\mathrm{C}$
- $\mathrm{NaN_3}(s) \rightarrow \mathrm{N}_2(g)$
- How much of $\mathrm{NaN_3}(s)$ must be decomposed to get $N_2$ gas at 1.15 atm ? & $26^o\mathrm{C}$ to occupy $36\mathrm{L}$ ?
- $\mathrm{NaN_3}(s)\rightarrow \text {very little volume}$
- $\mathrm{N}_2(g)\rightarrow \text {lot more volume}$

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<footer style = "font-size: 18px">Avogadro's hypothesis $\rightarrow$ Three gas laws $\rightarrow$ <span style = "color:blue"> Practical use </span> $\rightarrow$ Ideal gas equation of state $\rightarrow$ Thank you </footer>