Read the passage carefully and answer the question
The speed at which a chemical reaction takes place is called the rate of reaction. The rate of reaction depends on various factors like concentration of the reactants, temperature, etc. The relation between the rate of reaction and the concentration of reacting species is represented by the equation r = k[A]^x[B]^y, where x and y are the order of the reaction with respect to the reactants A and B, respectively. The overall order of the reaction is x + y. The rate of reaction can also be increased by the use of a catalyst which provides an alternate pathway of lower activation energy. It increases the rate of forward and backward reaction to an equal extent. It does not alter the Gibbs energy of the reaction.
Calculate the order of a reaction whose Rate = k[A]^1/2 [B]^3/2.

Consider the following statements for the order of a reaction and choose the correct statements.
(A). The order of a reaction is an experimental quantity.
(B). Order can be zero.
(C). Order can be fractional value.
(D). Order is applicable to elementary as well as complex reactions.
Choose the correct answer from the options given below :

Match List-I with List-II

List-I (Complex ion)	List-II (Hybridisation)
(A) \(\left[ CoF _6\right]^{3-}\)	(I) \(d^2 s p^3\)
(B) \(\left[ Co ( CN )_4\right]^{2-}\)	(II) \(s p^3 d^2\)
(C) \(\left[ FeCl _4\right]^{-}\)	(III) \(s p^3\)
(D)\(\left[ Co \left( C _2 O _4\right)_3\right]^{3-}\)	(IV) \(d s p^2\)

Choose the correct answer from the options given below:

The standard reduction potentials are given as:
\(\begin{array}{l}
E_{K^{+} / K}^{\circ}=-2.93 V \\
E_{Ag^{+} / Ag}^{\circ}=+0.80 V \\
E_{Cu^{2+} / Cu}^{\circ}=+0.34 V \\
E_{Ni^{2+} / Ni}^{\circ}=-0.25 V \\
E_{Li^{+} / Li}^{\circ}=-3.05 V
\end{array}\)
Arrange the following metals in increasing order of their reducing power:
A.K
B. Ag
C. Cu
D. Ni
E. Li
Choose the correct answer from the options given below:

Which type of isomerism is shown by the complex compounds?
\(\left[ Co \left( NH _3\right)_5 Br \right] SO _4\) and \(\left[ Co \left( NH _3\right)_3 SO _4\right]\)Br

When the electronic configuration of a transition metal element \(X\) in +3 oxidation state is \([ Ar ] 3 d^5\), what is its atomic number?

If an electrolyte on dissociation gives \(\nu_{+}\) cations and \(\nu_{-}\) anions, then its limiting molar conductivity is given by

Read the passage carefully and answer
When a metal is placed in a solution of its ions, the metal can lose electron and can go in the solution as ion or the metal ion in the solution can take electron from the electrode and get deposited as metal. Thus, the electrode acquires either positive or negative charge with respect to the solution leading to the development of a potential difference between the metal electrode and the solution. This potential difference is called the electrode potential of the metal. The electrode potential of a metal is a measure of relative tendency to undergo oxidation (loss of electron) or reduction (gain of electron). When the concentration of the ions in the solution is unity, the electrode potential is called standard electrode potential. The magni of potential depends upon the nature of electrode, concentration of ions in solution and the temperature. In a galvanic cell, the electrode at which oxidation occurs is known as anodic half-cell and the electrode at which reduction occurs is known as cathodic half cell. The emf of the cell in terms of standard reduction potential is given by \(E_{\text {cell }}^{\circ}=E_{\text {cathode }}^{\circ}-E_{\text {anode. }}^{\circ}\).The standard free energy change of the redox reaction taking place in the cell is related to \(E_{\text {cell }}^{\circ}\) by \(\Delta G^{\circ}=-n F E^{\circ}\). A redox reaction would occur spontaneously if the free energy change is negative. The equilibrium constant of the reaction is related to the standard free energy change by \(\Delta G^{\circ}=-R T \ln K\).
The measured potential for
\(A g ^{+}+ e ^{-} \rightarrow A g ( s )\)
does not change with

Arrange the following electrodes in decreasing order of the strength of the respective ions as reducing agent.
(A) \(Cu ^{2+}+2 e^{-} \rightarrow Cu (s) \quad E^{\circ}=0.34 V\)
(B) \(Sn ^{2+}+2 e^{-} \rightarrow \operatorname{Sn}(s) \quad E^{\circ}=-0.14 V\)
(C) \(AgBr ( s )+e^{-} \rightarrow Ag ( s )+ Br ^{-} \quad E^{\circ}=0.10 V\)
(D) \(Pb ^{2+}+2 e^{-} \rightarrow Pb (s) \quad E^{\circ}=-0.13 V\)
Choose the correct answer from the options given below

If \(y=x \log x\), then which of the following is correct ?

Answer the question on the basis of passage given below :
There are some deposits of nitrates and phosphates in the earth’s crust. Nitrates are more soluble in water. Nitrates are difficult to reduce under laboratory conditions, but microbes do it easily. Ammonia forms a large number of complexes with transition metals. Hybridisation easily explains the ease of sigma donation capability of NH₃ and PH₃. Phosphine is an inflammable gas, and it is prepared from white phosphorus.
Which of the following is the correct statement?

In a village, there are three mohallas A, B and C. 60\% farmers in mohalla A believe in new technology of agriculture, while in B it is 70\% and in C is 80\%.
District agricultural officer selects a farmer at random and he found that the farmer believed in new technology of agriculture, then the probability that he belongs to mohalla B is:

The degree of the differential equation \(\left(\frac{d y}{d x}\right)^3+\left(\frac{d^2 y}{d x^2}\right)^2=0\) is: