The specific conductance has the unit :

What is the value of ${\mathrm{pK}}_{\mathrm{b}} ({\mathrm{CH}}_3{\mathrm{COO}}^{-} )$ if ${\mathrm{\lambda }}_{\mathrm{m}}^0= 390 \& {\mathrm{\lambda }}_{\mathrm{m}} = 7.8$ for 0.04 of a ${\mathrm{CH}}_3\mathrm{COOH}$  at $25°\mathrm{C}$ ?

At $25°C$, the standard emf of cell having reactions involving two electron change is found to be 0.295 V. The equilibrium constant of the reaction is-

The number of faradays required to produce one mole of water from a hydrogen-oxygen fuel cell containing aqueous alkali as an electrolyte is-

How much current is necessary to produce $H_2$ gas at the rate of 1 $c{m}^3$ per second under STP ?

A current of 0.250 A is passed through 400 ml of a 2.0 M solution of NaCl for 35 minutes. What will be the pH of the solution after the current is turned off ?

During discharge of a lead storage cell, the density of sulphuric acid in the cell-

The cell reaction for the given cell is spontaneous if- 

$Pt(H_2,P_1 ) H^{+} \left(1M\right) \left|\right| H^{+} \left(1M\right) | Pt(H_2, P_2 )$

$\left(A\right) P_1 > P_2$

$\left(B\right) P_1 < P_2$

$\left(C\right) P_1 = P_2$

$\left(D\right) P_2 = 1 atm$

The standard electrode potentials (reduction) of Pt/Fe³⁺, Fe²⁺ and Pt/Sn⁴⁺, Sn²⁺ are + 0.77 V and + 0.15 V respectively at 25°C. The standard EMF of the reaction Sn⁴⁺ + 2Fe²⁺ → Sn²⁺ + 2Fe³⁺ is

In the following electrochemical cell, $M|M^{+} || X^{-}|X,$ the standard reduction potentials are $E{°}_{M+/M}= 0.52 V$ and $E{°}_{X/X^{-}} = 0.42 V at 25°C.$ Which one of the following statements is correct ?

Specific conductance of 0.01 M KCl solution is x $oh{m}^{-1}c{m}^{-1}$. When conductivity cell is filled with 0.01 M KCl the conductance observed is y $oh{m}^{-1}$. When the same cell is filled with 0.01 M$H_2 S{O}_4$ the observed conductance was $z oh{m}^{-1} c{m}^{-1}.$ Hence specific conductance of 0.01 M $H_2 S{O}_4$ is-

$F_2$ gas can’t be obtained by the electrolysis of any $F^{-1}$salt because-

Calculate the quantity of electricity (i.e. charge) delivered by a Daniel cell initially containing 1L each of $1 M C{u}^{2+}$ion and $1M Z{n}^{2+},$which is operated until its potential drops to 1V.
(Given : \(E_{Zn2+/Zn}^0 = -0.76V; E_{Cu2+/Cu}^0 = +0.34V\))

Some half cell reaction & their standard potential are given which combination would result in a cell with the largest potential.

$\left(i\right) A+e^{-} \to A^{-} E° = – 0.24$

$\left(ii\right) B^{-} + e^{-}\to B^{-2} E° = 1.25$

$\left(iii\right) C^{-} + 2^{e-} \to C^{-3} E{ }^{-}= – 1.25$

$\left(iv\right) D + 2^{e-} \to D^{-2} E° = 0.06$

$\left(v\right) E + 4^{e-}\to E^{-4} E° = 0.38$

A hydrogen electrode is immersed in a solution with pH = 0 (HCl). By how much will the potential (reduction) change if an equivalent amount of NaOH is added to the solution. $(Take p_{H_{2_{}}} = 1 atm) T = 298 K.$

The solubility product of silver iodide is $8.3 \times {10}^{-17}$and the standard potential (reduction) of Ag,$A{g}^{+}$ electrode is + 0.800 volts at ${25}^{°}C.$The standard potential of Ag, AgI/$I^{-}$ electrode (reduction) from these data is-

How much time is required for the complete decomposition of 2 moles of water using a current of 2 ampere-

The standard redox potentials $E^{\circ }$ of the following systems are-

System                                                                                    E° (volts)

$\left(i\right) \; \; <span\; class="math-tex">\backslash (MnO\_\{4\}^\{-\}+8\; H^\{+\}+5\; e\; \backslash rightarrow\; M\; n^\{2+\}+4\; H\_\{2\}O\backslash )</span>\; \; \; \; \; \; \; \; \; \; \; \; 1.51$

$\left(ii\right) S{n}^{4+}+ 2e \to S{n}^{2+} \; 0.15$

$\left(iii\right) C{r}_2{O_7}^{2-}+ 14H^{+} + 6e\to 2C{r}^{3+} + 7H_{2}O \; \; \; \; \; \; 1.33$

$\left(iv\right) C{e}^{4+} + e\to C{e}^{3+} \; \; 1.61$

The oxidising power of the various species decreases in the order-

Calculate the maximum work that can be obtained from the Daniell cell given below -

$Zn\left(s\right) | Z{n}^{2+} (aq) || C{u}^{2+ }(aq) | Cu\left(s\right).$

Given that $E_{Z{n}^{2+}/Zn}^{°}=-0.76 V and E_{C{u}^{2+}/Cu}^{°}=+0.34 V$

The metal that cannot be produced on reduction of its oxide by aluminium is :

We have taken a saturated solution of $AgBr, K_{sp}$ of AgBr is $12 \times {10}^{-14}.$If ${10}^{-7}$mole of $AgN{O}_3$ are added to 1 litre of this solution then the conductivity of this solution in terms of ${10}^{-7}$ $S{m}^{-1}$ units will be

$$\begin{gathered} [\lambda {°}_{\left(A{g}^{+}\right)}=4\times {10}^{-3}S{m}^{2}mo{l}^{-1} ; \\ \lambda {°}_{\left(B{r}^{-}\right)}=6\times {10}^{-3}S{m}^{2}mo{l}^{-1}, \\ \lambda {°}_{\left(N{O}_3^{-}\right)}=5\times {10}^{-3}S{m}^{2}mo{l}^{-1}] \end{gathered}$$

The electrode potential of Cu electrode dipped in 0.025 M CuS$O_4$ solution at 298 K is:

(standard reduction potential of Cu = 0.34 V)

The standard potentials, $E^{\circ }$, for the half reactions are as $Zn = Z{n}^{2+}+ 2e; E° = + 0.76 V$and $Fe = F{e}^{2+} + 2e ; E° = + 0.41$ V; the e.m.f. for the cell reaction, $F{e}^{2+}+ Zn = Z{n}^{2+}+ Fe is-$

Which of following cell can produce more electrical work.

The calomel electrode is reversible with respect to-

Zn amalgam is prepared by electrolysis of aqueous $ZnC{l}_2$ using Hg cathode (9 gm). How much current is to be passed through $ZnC{l}_2$ solution for 1000 seconds to prepare a Zn Amalgam with 25% Zn by wt. (Zn = 65.4)

The standard oxidation potentials of $Cu/C{u}^{2+}$and $C{u}^{+} /C{u}^{2+} are – 0.34V and – 0.16 V$respectively. The standard electrode potential of $C{u}^{+} /Cu$ would be :

Acidified water is electrolyzed using an inert electrode. The volume of gases liberated at

STP is 0.168L. The quantity of charge passed through the acidified water would be:

 $$\begin{gathered} {\mathrm{E}}^0 \mathrm{for} \mathrm{the} \mathrm{reaction} \\ \mathrm{Fe} + {\mathrm{Zn}}^{2+} = \mathrm{Zn} + {\mathrm{Fe}}^{2+} \mathrm{is} – 0.35 \mathrm{V}. \\ \mathrm{The} \mathrm{given} \mathrm{cell} \mathrm{reaction} \mathrm{is}- \end{gathered}$$ 

How much charge should be supplied to a cell for the electrolytic production of 245 gm $NaCl{O}_4$ from $NaCl{O}_3$ if the anode efficiency for the required reaction is 60%?