Match List I with List II

List-l	List-II
A. \(K _2 SO _4( aq )\) with \(60 \%\) dissociation	I. \(i = 3 . 7\)
B. \(K _3\left[ Fe ( CN )_6\right]( aq )\) with \(90 \%\) dissociation	II. \(i=1.8\)
C. \(AlCl _3( aq )\) with \(80 \%\) dissociation	III. \(i=2.2\)
D. \(K _2 HgI _4( aq )\) with \(40 \%\) dissociation	IV. \(i=3.4\)

Choose the correct answer from the options given below :

Reaction :
Benzene \(\xrightarrow[\text { Anhyd. } AlCl l _{ s } / CuCl ]{ CO _{ Cl } HCl } X\)
\(X\) in above reaction is

The common name and IUPAC name of the following compound, respectively, are

Arrange the following amines in the order of decreasing basic character in gaseous phase:
(A) \(\text{NH}_3\)
(B) \((\text{CH}_3)_3\text{N}\)
(C) \((\text{CH}_3)_2\text{NH}\)
(D) \(\text{CH}_3\text{NH}_2\)
Choose the correct answer from the options given below:

In the reaction below, identify the species undergoing oxidation and reduction.
H\(_2\)\(\mathrm{S}\)(g) + Cl\(_2\)(g) \(\rightarrow\) 2HCl(g) + S(s)

Read the passage carefully and answer the questions based on the passage:
The number of reacting species (atoms, ions or molecules) taking part in an elementary reaction, which must collide simultaneously in order to bring about a chemical reaction is called molecularity of a reaction. In the rate equation Rate \(=k[\mathrm{~A}]^x[\mathrm{~B}]^y\)
\(x\) and \(y\) indicate how sensitive the rate is to the change in concentration of A and B, respectively. Sum of these exponents, i.e., \(x +y\) gives the overall order of a reaction where \(x\) and \(y\) represent the order with respect to the reactants A and B respectively. Hence, the sum of powers of the concentration of the reactants in the rate law expression is called the order of that chemical reaction. For a first order reaction, the concentration of the reactant varies as \([\mathrm{R}]=[\mathrm{R}]_0 e^{-k t}\)
The units of first and zero order rate constant of reactions are respectively:

"Answer the question on basis of passage given below :
Carboxylic acids are weaker than mineral acids, but they are stronger acids than alcohols and many simple phenols (\(\text{pKa}\) is ~ 16 for ethanol and 10 for phenol). The higher acidity of carboxylic acids as compared to phenols can be understood similarly. The conjugate base of carboxylic acid, a carboxylate ion, is stabilised by two equivalent resonance structures in which the negative charge is at the more electronegative oxygen atom. The conjugate base of phenol, a phenoxide ion, has non-equivalent resonance structures in which the negative charge is at the less electronegative carbon atom. Further, the negative charge is delocalised over two electronegative oxygen atoms in carboxylate ion whereas it is less effectively delocalised over one oxygen atom and less electronegative carbon atoms in phenoxide ion. Thus, the carboxylate ion is more estabilised than phenoxide ion, so carboxylic acids are more acidic than phenols.
Effect of substituents on the acidity of carboxylic acids: substituents may affect the stabliity of the conjugate base and thus, also affect the acidity of the carboxylic acids. Electron withdrawing group increase the acidity of carboxylic acids by stabilising the conjugate base through delocalisation of the negative charge by inductive and/or resonance effects. Conversely, electron donating groups decrease the acidity by destabilising the conjugate base.
The weakest among the following acid is :"

The area of the triangle with vertices \((1,4),(2,7)\) and \((4,13)\) is:

The major product formed when acetanilide undergoes bromination in presence of acetic acid is:

For (i) \(I^-\) (ii) \(Cl^-\)(iii) \(Br^-\), the usual increasing order of nucleophilicities would be

The product of the following chemical reaction is
Glucose \(\xrightarrow{ Br _2 \text { water }}\)

Radiation of frequency \(2 v _0\) incident on a metal with threshold frequency \(v _0\) results in maximum kinetic energy of photoelectrons as :

If \(\int_0^a 3 x^2 d x=27\), then value of \(a\) is :