\(\underset{(\mathrm{L} x)}{\mathrm{CaCO}_3} \rightleftharpoons \underset{(x)}{\rightleftharpoons} \mathrm{CaO}_{(\mathrm{s})}+\underset{(x)}{\mathrm{CO}_{2(\mathrm{~g})}}\)
K_c = [CO₂]
\(K_c=\frac{x}{V}\)
So, \(K_c \propto \frac{1}{V}\) If V increases K_c wil decrease; As K_c is a constant x will increase and hence the yield of the product will increase. Similarly if V decreases the yield of the product will also decrease.

aliphatic open chain.
Propane - \(\mathrm{CH}_3-\mathrm{CH}_2-\mathrm{CH}_3\)
Propylene - \(\mathrm{CH}_3-\mathrm{CH}=\mathrm{CH}_2\)

4-methyl - 2-pentene

(i) Unsaturated open chain compound
(ii) saturated open chain compound
(iii) aromatic benzenoid compound
(iv) alicyclic compound

No of e^o in C₂ ^2- : 6 + 6 + 2 = 14 e^o
Electronic configuration of C₂ ^2- ion is:
σ_1s², σ*_1s² ,σ_2s² , σ_2s² ,π2py² = π2px² , π2py²
Bond order = 1/2 (N_b - N_a)
= 1/2(10 - 4) = 3

(i) \(log\cfrac { { K }_{ 2 } }{ { K }_{ 1 } } =\cfrac { \Delta { H }^{ o } }{ 2.303R } \left[ \cfrac { { T }_{ 2 }{ T }_{ 1 } }{ { T }_{ 2 }{ T }_{ 1 } } \right] \)
(ii)  \({ K }_{ C }=\cfrac { \left[ { Cl }_{ 2 }\left( g \right) \right] ^{ 2 }\left[ { H }_{ 21 }O(g) \right] ^{ 2 } }{ \left[ HCl(g) \right] ^{ 4 } } \)

The formation of photochemical smog can be suppressed by preventing the release of nitrogen oxide and hydrocarbons into the atmosphere from the motor vehicles by using catalytic convertors in engines. Plantation of certain trees like Pinus, Pyrus Querus vitus and Juniparus can metabolise nitrogen oxide.

(i) \(H-C\equiv C-CH_{ 2 }-\underset { \underset { OH }{ | } }{ CH } -{ CH }_{ 3 }\)

Greater the polarization effect, greater will be covalent character imported into the ionic bond. The general trend in the polarizing power of cations is Li⁺ > Na⁺ > K⁺ > Rb⁺> Cs⁺
\(\therefore\)Their covalent charter: LiCI > NaCl > KCl > RbCl > CsCl

According to him, "the partial pressure of the gas in vapour phase (vapour pressure of the solute) is directly proportional to the mole fraction(x) of the gaseous solute in the solution at low concentrations". is statement is known as Henry's law.
p_solute \(\infty \)Xsolute in solution
p_solute = K_Hx_{solute in solution} 
Here, P_solute represents the partial pressure of the gas in vapour state which is commonly called as vapour pressure.

Halo arenes do not undergo nucleophilic substitution reaction readily is due to C-X bond in aryl halide is short and strong and also the aromatic ring isa centre of high electron density.
The halogen of haloarenes can be substituted by OH^-, NH₂^-, or CN^- with appropriate nucleophilic reagents at high temperature and pressure.

CH₃CH₂CH₂COONa + NaOH \(\overset { CaO }{ \underset { \Delta }{ \rightarrow } } \)CH₃CH₂ - CH₃+Na₂CO₃
Sodium salt of butanaic acid           Propane
Heating sodium salt of butanoic acid (Sodium butanoate) with soda lime gives propane.

The resonance is a chemical phenomenon which is observed in certain organic compounds possessing double bonds at a suitable position. Certain organic compounds can be represented by more than one structure and they differ only in the position of
bonding and lone pair of electrons. Such structures are called resonance structures (canonical structures) and this phenomenon is called resonance. This phenomenon is also called mesomerism or mesomeric effect.
For example, the structure of aromatic compounds such as benzene and conjugated systems tike 1,3 - butadiene cannot be represented by a single structure, and their observed properties can be explained on the basis of a resonance hybrid.
In 1, 3 buta diene, it is expected that the bond between C₁ - C₂ and C₃ - C₄ should be shorter than that of C₂ - C₃, but the observed bond lengths are of same. This property cannot be explained by a simple structure in which two \(\pi\) bonds localised between C₁ - C₂ and C₃ - C₄ . Actually the \(\pi\) electrons are delocalised

These resonating structures are called canonical forms and the actual structure lies between these three resonating strucfures, and is called a resonance hybrid. The resonance hybrid is represented
Similar to the other electron displacement effect, mesomeric effect is also classified into positive mesomeric effect (+M or +R) and negative mesomeric effect (-M of -R) based on the nature of the functional group present adjacent to the multiple bond.
Positive Mesomeric Effect :
Positive resonance effect occurs, when the electrons move away from substituent attached to the conjugated system. It occurs, if the electron releasing substituents are attached to the conjugated system. In such cases, the attached group has a tendency to release electrons through resonance. These electron releasing groups are usually denoted as +R or +M groups.
Examples : -OH, -SH, -OR, -SR, -NH₂, -O- etc...
Negative Mesomeric Effect :
Negative resonance effect occurs, when the electrons move towards the substituent attached to the conjugated system. It occurs if the electron withdrawing substituents are attached to the conjugated system.

In such cases, the attached group has a tendency to withdraw electrons through resonance. These electron withdrawing groups are usually denoted as -R or -M groups.
Examples : NO₂, > C = O, -COOH, -C = N etc......
Resonance is useful in explaining certain properties such as acidity oi phenol. The phenoxide ion is more stabilised than phenol by resonance effect (+M effect) and hencp resonance tavours ionisation of phenol to form H⁺ and shows acidity.
The structures shows that there is a charge separation in the resonance structure of phenol which needs energy, where as there is no such hybrid structures in the case of phenoxide ion. This increased stability accounts for the acidic character of phenol.

Two solutions having same osmotic pressure at a given temperature are called isotonic solutions.

No.of moles ; n = \(\frac{\mathrm{m}}{\mathrm{M}}=\frac{5.6}{56}=0.1 \mathrm{~mol}\)
(i) V = 500 ml = \(\frac{500}{1000}=0.5 \mathrm{~L} \)
Molarity = \(\frac{\mathrm{n}}{\mathrm{v}}=\frac{0.1}{0.5}=0.2 \mathrm{M} \)
(ii) V = IL 
Molarity = \(\frac{\mathrm{n}}{\mathrm{v}}=\frac{0.1}{1}=0.1 \mathrm{M} \)

\( \mathrm{H}_{2(\mathrm{~g})}+\mathrm{I}_{2(\mathrm{~g})} \rightleftharpoons 2 \mathrm{HI}_{(\mathrm{g})} \)
\(\mathrm{K}_{\mathrm{c}}=\frac{4 x^{2}}{(a-x)(b-x)}\)
This expression doesn't involve, V. So, increase or decrease of volume will not affect the equilibrium and hence the yield of the product.

ΔH_f⁰ CO₂ = -393.5 kJ mol^-1
ΔH_f⁰ CO = -111.31 kJ mol^-1
ΔH_f⁰ (H₂O) = - 242 kJ mol^-1
CO₂(g) + H₂(g) - CO(g) + H₂O(g)
ΔH_f⁰ = ?
ΔH_f⁰ = Σ(ΔH_f⁰)_products-Σ(ΔH_f⁰)_reactions
ΔH_f⁰ = [ΔH_f⁰(CO) + ΔH_f⁰(H₂O)] - [ΔH_f⁰(CO₂) + ΔH_f⁰(H₂)]
ΔH_f⁰ = [-111.31 + (-242)] - [-393.5 + (0)]
ΔH_f⁰ = [-353.31] + 393.5
ΔH_f⁰ = 40.19
ΔH_f⁰ = +40.19 kJ mol^-1.

Noble gases: Ioniation energy ranging from 2372 KJmol^-1 to 1037 kJ mol^-1.
For element X, the IE₁ value is in the range of noble gas, moreover for this element both IE₁ and IE₂ are higher and hence X is the noble gas.
For Y, the first ionisation energy is low and second ionisation energy is very high and hence Y is most reactive metal. For Z, both IE₁ and IE₂ are higher and hence it is least reactive.

Electronic configuration of Fe³⁺ : 1s² 2s² 2p⁶ 3s² 3p⁶ 4s⁰ 3d⁵
Electronic configuration of Ni²⁺ : 1s² 2s² 2p⁶ 3s² 3p⁶ 4s⁰ 3d⁸
Fe³⁺ has stable 3d⁵ half filled configuration.

The enthalpy change of a reaction either at constant volume or constant pressure is the same whether it takes place in a single or multiple steps provided the initial and final states are same.

The solubility product of NaCl is lower than that of NaOH. The more soluble a substance is, the higher the K_sp value it has In aqueous solution NaOH gives OH^- ions. It can be solvated by establishing H-bonds with water molecules. So it is more water soluble.

(i) ground state :

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

\(​​\upharpoonleft \)

This type of electronic configuration have ten possible arrangement (i.e. Half filled configuration is More).

Gases are very less denser. They have negligible intermolecular forces of attraction between the molecules. They are in continuous kinetic motion. So they won't settle at the bottom due to gravitational forces. The material that is most dense will sink to the bottom; the less denser will go up.

Average atomic mass
= \(\frac { (78.99\times 23.99)+(10\times 24.99)+(11.01\times 25.98) }{ 100 } \)
= \(\frac { 2430.9 }{ 100 } \)
= 24.31 u

''The relative atomic mass is defined as the ratio of the average atomic mass factor to the unified atomic mass unit''.

Ions of different elements having the same number of electrons are called isoelectronic ions.

Ions of different elements	Na+	Mg+2	Al+3	F-	O2-	N3-
No. of electrons	10	10	10	10	10	10