How much charge is required for the reduction of 0.05 moles of \(MnO _4^{-}\) to \(MnO _2\)?

Match List-I with List-II

List-I (Structure of Protein)	List-II (Function)
(A) Primary Structure	(I) Gives rise to Fibrous and Globular Proteins
(B) Secondary structure	(II) Sequence of amino acid
(C) Tertiary Structure	(III) shape of polypeptide chain
(D) Quaternary Structure	(IV) Spatial arrangement of sub-units

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Match the statement of set of orbitals given in List-I with orbitals and energy separation given in List-II

List – I (Statements)	List-II (Orbitals and energy separation)
(A) \(t_{2 g}\) set of orbitals in octahedral crystal field and energy separation from barycentre	(I) \(d_{x^2-y^2}, d_{z^2}\) and \(3 / 5 \Delta_t\)
(B) \(e_g\) set of orbitals in octahedral crystal field and energy separation from barycentre	(II) \(d_{x y}, d_{x z}, d_{y z}\) and \(2 / 5 \Delta_t\)
(C) \(t_2\) set of orbitals in tetrahedral crystal field and energy separation from barycentre	(III) \(d_{x^2-y^2}, d_{z^2}\) and \(3 / 5 \Delta_0\)
(D) \(e\) set of orbitals in tetrahedral crystal field and energy separation from barycentre	(IV) \(d_{x y}, d_{x z}, d_{y z}\) and \(2 / 5 \Delta_0\)

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0.01 molal aqueous solutions of strong electrolytes \(NaCl , KCl , MgSO _4\) and \(K _2 SO _4\) are prepared.Which of the following statements is correct regarding their osmotic pressure ? (Assume complete dissociation of solute particles)

The resistance of 1N solution of four different electrolytes are given below. Arrange them in increasing order of their equivalent conductance values if the same conductivity cell was used to measure the resistance of all the electrolytic solutions:
(A) 250 ohm
(B) 150 ohm
(C) 50 ohm
(D) 280 ohm
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Arrange the following compounds in increasing order of reactivity towards Nucleophilic Substitution Reaction
(A) Chlorobenzene
(B) 4- Nitrochlorobenzene
(C) 2,4 - Dinitrochlorobenzene
(D) 2,4,6-Trinitrochloronitrobenzene
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The presence or absence of hydroxyl group on which carbon is ribose sugar differentiate RNA and DNA?

In the formation of a Leclanche cell, the space between electrodes is filled with:
(A) \(ZnCl _2\)
(B) \(NH _4 Cl\)
(C) \(AlCl _3\)
(D) ZnS
(E) \(NH _4 NO _3\)
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Identify the correct IUPAC name of the given compound:

What sum of money is needed to invest now, so as to get ₹5000 at the beginning of every month forever, if the money is worth \(6\%\) per annum compounded monthly?

The puffed up appearance of dough is due to the production of:

From a container full of milk, 10 liters (1) was drawn and replaced by water. This process is repeated one more time. The ratio of quantity of milk and water left in the container is \(4: 5\). Then the capacity of the container is :

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 standard Oxidation potential \(E^0\) for the half cell reactions are
\(Zn \rightarrow Zn ^{2+}+2 e^{-}: E^0=+0.76 V\)
\(Fe \rightarrow Fe ^{2+}+2 e^{-}: E^0=+0.41 V\)
The emf of cell \(Fe ^{2+}+ Zn \rightarrow Zn ^{2+}+ Fe\) is