The major product of the following reaction is :

The major product of the following reaction is :

An aromatic compound 'A' having molecular formula C7H6O2 on treating with aqueous ammonia and heating forms compound 'B'. The compound 'B' on reaction with molecular bromine and potassium hydroxide provides compound 'C' having molecular formula C6H7N.. The structure of 'A' is

The major product obtained in the following reaction is :

The major product formed in the reaction given below will be :

The major product of following reaction is :

Arrange the following amines in the decreasing order of basicity :

Given CO3+ + e– $$\to$$ CO2+ ; Eo = + 1.81 V Pb4+ + 2e– $$\to$$ Pb2+ ; Eo = + 1.67 V Ce4+ + e– $$\to$$ Ce3+ ; Eo = + 1.61 V Bi3+ + 3e– $$\to$$ Bi ; Eo = + 0.20 V Oxidizing power of the species will increase in the order :

Which one of the following graphs between molar conductivity ($${\Lambda }_m$$) versus $$\sqrt{C}$$ is correct ?

Consider the statements S1 and S2 S1 : Conductivity always increases with decrease in the concentration of electrolyte. S2 : Molar conductivity always increases with decrease in the concentration of electrolyte. The correct option among the following is :

A solution of Ni(NO3)2 is electrolysed between platinum electrodes using 0.1 Faraday electricity. How many mole of Ni will be deposited at the cathode?

The standard Gibbs energy for the given cell reaction in kJ mol–1 at 298 K is : Zn(s) + Cu2+ (aq) $$\to$$ Zn2+ (aq) + Cu (s), E° = 2 V at 298 K (Faraday's constant, F = 96000 C mol–1)

Calculate the standard cell potential in (V) of the cell in which following reaction takes place : Fe2+(aq) + Ag+(aq) $$\to$$ Fe3+(aq) + Ag (s) Given that $$E_{A{g}^{+}/Ag}^o=xV$$ $$E_{F{e}^{2+}/Fe}^o=yV$$ $$E_{F{e}^{3+}/Fe}^o=zV$$

$${\wedge }_m^{\circ }$$ for NaCl, HCl and NaA are 126.4, 425.9 and 100.5 S cm2 mol–1, respectively. If the conductivity of 0.001 M HA is- 5 $$\times$$ 10–5 S cm–1, degree of dissociation of HA is -

The standard electrode potential $$E^o$$ and its temperature coefficient \left( {{{d{E^o }} \over {dT}}} \right) for a cell are 2V and $$-$$ 5 $$\times$$ 10$$-$$4 VK$$-$$1 at 300 K respectively. The cell reaction is Zn(s) + Cu2+ (aq) \buildrel \, \over \longrightarrow Zn2+ (aq) + Cu(s) The standard reaction enthalpy ($$\Delta$$rH$${}^o$$) at 300 K in kJ mol–1 is, [Use R = 8 JK–1 mol–1 and F = 96,000C mol–1]

The anodic half-cell of lead-acid battery is recharged using electricity of 0.05 Faraday. The amount of PbSO4 electrolyzed in g during the process is : (Molar mass of PbSO4 = 303 g mol$$-$$1)

Given that $${E^{\Theta }}_{O_2/H_{2}O}=1.23V$$ ; $${E^{\Theta }}_{S_2{O}_8^{2-}/S{O}_4^{2-}}=2.05V$$ $${E^{\Theta }}_{B{r}_2/B{r}^{-}}=1.09V$$ $${E^{\Theta }}_{A{u}^{3+}/Au}=1.4V$$ The strongest oxidizing agent is :

If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s) + Cu2+ (aq) $$\rightleftharpoons$$ Zn2+(aq) + Cu(s) at 300 K is approximately, (R = 8 JK$$-$$1mol$$-$$1, F = 96000 C mol$$-$$1)

Consider the following reduction processes : Zn2+ + 2e– $$\to$$ Zn(s) ; Eo = – 0.76 V Ca2+ + 2e– $$\to$$ Ca(s); Eo = –2.87 V Mg2+ + 2e– $$\to$$ Mg(s) ; Eo = – 2.36 V Ni2 + 2e– $$\to$$ Ni(s) ; Eo = – 0.25 The reducing power of the metals increases in the order :

For the cell Zn(s) |Zn2+ (aq)| |Mx+ (aq)| M(s), different half cells and their standard electrode potentials are given below : .tg {border-collapse:collapse;border-spacing:0;} .tg td{font-family:Arial, sans-serif;font-size:14px;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg th{font-family:Arial, sans-serif;font-size:14px;font-weight:normal;padding:10px 5px;border-style:solid;border-width:1px;overflow:hidden;word-break:normal;border-color:black;} .tg .tg-a0j4{font-size:18px;text-align:left} .tg .tg-nx8p{font-size:18px;text-align:left;vertical-align:top} Mx+ (aq)/M(s) Au3+(aq)/Au(s) Ag+(aq)/Ag(s) Fe3+(aq)/Fe2+ (aq) Fe2+(aq)/Fe(s) E0Mx+/M/(V) 1.40 0.80 0.77 $$-$$0.44 If $$E_{z{n}^{2+}/zn}^0$$ = $$-$$ 0.76 V, which cathode will give maximum value of Eocell per electron transferred?