chemistry-class-11-unit-05-chapter-07-states-of-matter-gases-and-liquids-l-7-8-t-hqtip-bzc

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-7 </Success>
### <primary style="font-size:24px"> Numerical </primary>
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- What is the density in $\mathrm {g~ L}^{-1}$ of ammonia at $0 { } ^oC$ and 1 atm of the gas in a 1.000 L bulbs weights 0.672g at 23 $^{0}C$ and 733.4 mm $H_g$ pressure
 
- **Solution**

- $PV = n R T$

- $n =\frac{m}{M}\quad  PV = \frac{m}{M} \mathrm {RT} $

- $P = \frac{1}M{}.\frac{m}{V}. RT$

- $\frac{m}{V} \rightarrow \text {density}$
	
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<footer style = "font-size: 18px">Numerical $\rightarrow$ Numerical $\rightarrow$ <span style = "color:blue"> Numerical </span> $\rightarrow$ Numerical $\rightarrow$ Numerical </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-7 </Success>
### <primary style="font-size:24px"> Numerical </primary>
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- **Solution**
- $P = \frac {\rho R T }{M}$

- $\text {P = 1 atm}$

- $T = 25^ oC = 298 K$

- $V = 1.000~ L$

- $m = 0.672\mathrm {~ g} /M_{NH_3} = 17\mathrm ~ g~ {mol}^{-1}$

- $\mathrm {\rho = 733.4~ mm ~ Hg}$

- $P\left\\{\begin{array}{l}\text { bar } \\\ \text { atm } \\\ \text { mm Hg/torr}\end{array}\right.$

- $760 \mathrm {~ mm ~ Hg} - 1 \text {~ atm}$

- $733 \mathrm {~ m ~ Hg} - ? \text {~ atm}$

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<footer style = "font-size: 18px">Numerical $\rightarrow$ Numerical $\rightarrow$ <span style = "color:blue"> Numerical </span> $\rightarrow$ Numerical $\rightarrow$ Numerical </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-7 </Success>
### <primary style="font-size:24px"> Numerical </primary>
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- When $NO_2$ is cooled to room temprature , some of it reacts to form a dimer , $N_2 O_4$, through the reaction $2 NO_2 (g) \rightarrow N_2O_4 (g)$ suppose $15.2 g$ of $NO_2$ is placed in a $10.0 L$ flask at high temprature and the flask is cooled to $25 ^{o}C.$ What partial pressures and mole fractions of $NO_2$ and $N_2O_4$ are present

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<footer style = "font-size: 18px">Numerical $\rightarrow$ Numerical $\rightarrow$ <span style = "color:blue"> Numerical </span> $\rightarrow$ Numerical $\rightarrow$ Numerical </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-7 </Success>
### <primary style="font-size:24px"> Numerical </primary>
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- **Solution**
- $\mathrm{NO}_2\left(T_h\right)(Initial) \xrightarrow[\text { cooled }]{ }\mathrm {NO}_2 + \mathrm {N}_2\mathrm{O}_4\left (T_e\right)(Funal)$

- $\text {law T:} 2~ NO_2(g)\rightarrow N_2 ~ O_4(g)$

- $\mathrm {n} = 15.2\mathrm {~ g ~ of} ~ NO_2\quad (n_{NO_2}^o)$

- $\ M_{NO_2} = 46 \mathrm {~ g ~ mol}^{-1}$

- $n^f =\ n_{NO_2}^f +2 \ n_{N_2O_4}^f = n^0=\ n_{NO_2}^0 $

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<footer style = "font-size: 18px">Numerical $\rightarrow$ Numerical $\rightarrow$ <span style = "color:blue"> Numerical </span> $\rightarrow$ Numerical $\rightarrow$ Numerical </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-7 </Success>
### <primary style="font-size:24px"> Numerical </primary>
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- **Solution**

- $P_{\text {total}} = 0.500 \text { atm }$

- $P=\frac{n_{NO_2}^{f} R T}{V}+\frac{n_{N_2 O_4} R T}{V}$

- $P= P_{NO_2} + P_{N_2O_4}$

- $ V = 10.0 ~ L / ~ T = 25^oC = 298 ~ K$

- $R = 0.082 \text { L atm  K }^{-1} \mathrm {~ mol}^{-1}$

- $R= 0.500 \text {~ atm}=\left(\frac{RT}{V}\right)$

- $\left\\{n_{NO_2}^f + n_{N_2O_4}^f\right\\}$

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<footer style = "font-size: 18px">Numerical $\rightarrow$ Numerical $\rightarrow$ <span style = "color:blue"> Numerical </span> $\rightarrow$ Numerical $\rightarrow$ Numerical </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-7 </Success>
### <primary style="font-size:24px"> Numerical </primary>
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- Automobile air bags are inflated by nitrogen gas generated by the rapid decomposition of sodium azide

- $N_a N_3 (s) : 2 N_a N_3 (s) \rightarrow 2N_a (s) + 3N_2 (g)$

- If an air bag has a volume of 36 L and is to be filled with nitrogen gas at 1.15 atm and $26^oC$ , how many grams of $N_a N_3$ , must be decomposed

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<footer style = "font-size: 18px">Numerical $\rightarrow$ Numerical $\rightarrow$ <span style = "color:blue"> Numerical </span> $\rightarrow$ Numerical $\rightarrow$ Numerical </footer>

### <Success style="font-size:25px"> States Of Matter Gases And Liquids L-7 </Success>
### <primary style="font-size:24px"> Molar volume </primary>
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- $\text {Molar volume at} ~ 0^{o}C ~ (273K) \text {and 1 atm}$

- $\quad\text {Molecule} \hspace {0.5cm}\text {Volume}$

- $2 e^{-}~ ~ \left[\begin{array}{ll}\mathrm{H}_2 &\quad22.415 \\\ \mathrm{H}_2 & \quad 22.428\end{array}\right.$

- $10 e^{-} \left[\begin{array}{ll}\mathrm{NH}_3 & 22.077 \\\ \mathrm{CH}_4 & 22.360 \\\ \mathrm{Ne} & 22.428\end{array}\right.$

- $14 e^{-}\left[\begin{array}{ll}\mathrm{C}_2 \mathrm{H}_2 & 22.274 \\\ \mathrm{CO} & 22.405\end{array}\right.$

- $\text {Molar volume close to 22.4 L but not equal}$

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<footer style = "font-size: 18px">Numerical $\rightarrow$ Numerical $\rightarrow$ <span style = "color:blue"> Molar volume </span> $\rightarrow$ Intermolecular frocess $\rightarrow$ Real Gas P-V behavior </footer>