Here is the list of all Gaseous State Class 11 Formulas. This formula list is very important to revise before your JEE Main, Advanced or NEET Exam.
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All Gaseous State Class 11 Formulas Stoichiometry Formulas Class 11
Temperature Scale :
$\frac{ C – O }{100-0}=\frac{ K -273}{373-273}=\frac{ F -32}{212-32}=\frac{ R – R ( O )}{ R (100)- R ( O )}$
Here, $R =$ Temp. on unknown scale.
Boyle’s law and measurement of pressure:
At constant temperature,
$V \alpha \frac{1}{ P }$
$P _{1} V _{1}= P _{2} V _{2}$
Charles law:
At constant pressure,
$V \propto T$, OR
$\frac{V_{1}}{T_{1}}=\frac{V_{2}}{T_{2}}$
Gay-lussac’s law:
At constant volume,
$\quad P \alpha T$
$\frac{ P _{1}}{ T _{1}}=\frac{ P _{2}}{ T _{2}} \rightarrow$ temp on absolute scale
Ideal gas Equation:
$PV = nRT$
$PV =\frac{ w }{ m } RT$ OR $P =\frac{ d }{ m } RT$ OR $Pm = dRT$
Daltons law of partial pressure:
$P _{1}=\frac{ n _{1} RT }{ v }, \quad P _{2}=\frac{ n _{2} RT }{ v }, \quad P _{3}=\frac{ n _{3} RT }{ v }$ and so on.
Total pressure $= P _{1}+ P _{2}+ P _{3}+\ldots \ldots .$
Partial pressure $=$ mole fraction $X$ Total pressure.
Amagat’s law of partial volume:
$V = V _{1}+ V _{2}+ V _{3}+\ldots \ldots .$
Average molecular mass of gaseous mixture:
$M _{ mx }=\frac{\text { Total mass of mixture }}{\text { Total no. of moles in mixture }}$ $=\frac{ n _{1} M _{1}+ n _{2} M _{2}+ n _{3} M _{3}}{ n _{1}+ n _{2}+ n _{3}}$
Graham’s Law:
Rate of diffusion r $\propto \frac{1}{\sqrt{ d }}$ ; $d =$ density of gas
$\frac{r_{1}}{r_{2}}=\frac{\sqrt{d_{2}}}{\sqrt{d_{1}}}=\frac{\sqrt{M_{2}}}{\sqrt{M_{1}}}=\sqrt{\frac{V \cdot D_{2}}{V \cdot D_{1}}}$
Kinetic Theory of Gases:
- $PV =\frac{1}{3} mN \overline{ U ^{2}} \quad$ Kinetic equation of gases
- Average K.E. for one mole $=N_{A}\left(\frac{1}{2} m \bar{U}^{2}\right)=\frac{3}{2} K N_{A} T=\frac{3}{2} R T$
- Root mean suqare speed
$U_{ rms }=\sqrt{\frac{3 RT }{ M }}$
molar mass must be in kg/mole. - Average speed
$U _{ av }= U _{1}+ U _{2}+ U _{3}+\ldots \ldots \ldots \ldots U _{ N }$
$U_{\text {avg. }}=\sqrt{\frac{8 R T}{\pi M}}=\sqrt{\frac{8 K T}{\pi m}}$
$K$ is Boltzmman constant - Most probable speed
$U_{ MPS }=\sqrt{\frac{2 RT }{ M }}=\sqrt{\frac{2 KT }{ m }}$
Vander wall’s equation:
$\left(P+\frac{a n^{2}}{v^{2}}\right)(v-n b)=n R T$
Critical constants:
$V_{c}=3 b$ ,
$P_{c}=\frac{a}{27 b^{2}}$,
$T _{ c }=\frac{8 a }{27 Rb }$
Vander wall equation in virial form :
$z=\left(1+\frac{b}{V_{m}}+\frac{b^{2}}{V_{m}^{2}}+\frac{b^{3}}{V_{m}^{3}}+\ldots \ldots \ldots\right)-\frac{a}{V_{m} R T}$ $=1+\frac{1}{V_{m}}\left(b-\frac{a}{R T}\right)+\frac{b^{2}}{V_{m}^{2}}+\frac{b^{3}}{V_{m}^{3}}+\ldots \ldots \ldots \ldots \ldots$
Reduced Equation of state:
$\left(P_{r}+\frac{3}{V_{r}^{2}}\right)\left(3 V_{r}-1\right)=8 T_{r}$
At “Study Material Center” you will get all the important exam related study material, such as Notes, Study Material, Formula bank, Previous Year Chapterwise Questions etc.
Class 11 Chemistry Formulas
- Chemical Bonding and Molecular Structure
- Chemical Equilibrium
- Classification of Elements and Periodicity in Properties
- Gaseous State
- Ionic Equilibrium
- P Block
- S Block
- Stoichiometry
- Structure of Atom
- Thermodynamics
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