Galvanic Cells

Consider the following equation for an electrochemical cell reaction. Which of the following changes in condition will increase the cell voltage? ${\mathrm{H}}_2\left(\mathrm{g}\right)+{\mathrm{PbCl}}_2\left(\mathrm{s}\right)\to \mathrm{Pb}\left(\mathrm{s}\right)+2\mathrm{HCl}\left(\mathrm{aq}\right)$
(I) Dissolve concentrated ${\mathrm{HClO}}_4$ in the cell solution
(II) Increase the pressure of ${\mathrm{H}}_2\left(\mathrm{g}\right)$
(III) Increase the amount of $\mathrm{Pb}\left(\mathrm{s}\right)$

A hypothetical electrochemical cell is $\mathrm{A}/{\mathrm{A}}^{+}\left(\mathrm{x} \mathrm{M}\right)\parallel {\mathrm{B}}^{+}\left(\mathrm{y} \mathrm{M}\right)/\mathrm{B}$. The emf measured is $+0.20 \mathrm{V}$. The cell reaction is 

Choose the correct statement for galvanic cell

Anode in the galvanic cell is:

When an aqueous solution of ${\mathrm{CuCl}}_2$ is electrolysed using Pt inert electrodes, the reaction at cathode and anode respectively are

A variable, opposite external potential (E_ext) is applied to the cell

$\mathrm{Zn}\left|{\mathrm{Zn}}^{2+} (1 \mathrm{M}) \left|\right| {\mathrm{Cu}}^{2+} (1 \mathrm{M}) \right| \mathrm{Cu}$, of potential $1.1 \mathrm{V}$. When ${\mathrm{E}}_{\mathrm{ext}}<1.1 \mathrm{V}$ and ${\mathrm{E}}_{\text{ext }}>1.1 \mathrm{V}$, respectively electrons flow from :

Which of the following statements is/are true for an electrochemical cell?

For the given cell: $\mathrm{Mg} \overline{){\mathrm{Mg}}^{2+}\parallel {\mathrm{Cu}}^{2+}\overline{) \mathrm{Cu}}}$
 

In a galvanic cell, which one of the following statement is not correct?

Which of the following statements is false?
 

Which of the following statements is true for the electrochemical Daniell cell?

Among the following, which reaction take place at anode?

What will happen if dil. ${\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4$ is electrolysed between Pt electrode?

The electrode potential, $\mathrm{E}°$ , for the reduction of $\mathrm{M}\mathrm{n}{\mathrm{O}}_4^{-}$ to $\mathrm{M}{\mathrm{n}}^{2+}$ in acidic medium is +1.51 V. Which of the following metal(s) will be oxidised? The reduction reactions and standard electrode potentials for $\mathrm{Z}{\mathrm{n}}^{2+},\mathrm{A}{\mathrm{g}}^{+}$ and $\mathrm{A}{\mathrm{u}}^{+}$ are given as

$\mathrm{Z}{\mathrm{n}}_{\left(\mathrm{a}\mathrm{q}\right)}^{2+}+2{\mathrm{e}}^{-}\to \mathrm{Z}{\mathrm{n}}_{\left(\mathrm{s}\right)},\mathrm{E}°=-0.762\mathrm{V}$

$\mathrm{A}{\mathrm{g}}_{\left(\mathrm{a}\mathrm{q}\right)}^{+}+{\mathrm{e}}^{-}\rightleftharpoons \mathrm{A}{\mathrm{g}}_{\left(s\right)},\mathrm{E}°=+0.80\mathrm{V}$

$\mathrm{A}{\mathrm{u}}_{\left(\mathrm{a}\mathrm{q}\right)}^{+}+{\mathrm{e}}^{-}\rightleftharpoons \mathrm{A}{\mathrm{u}}_{\left(\mathrm{s}\right)},\mathrm{E}°=+1.69\mathrm{V}$

A hypothetical electrochemical cell is shown below

$\mathrm{A}\left|{\mathrm{A}}^{+}\right(\mathrm{x}\mathrm{M}\left)\right|\left|{\mathrm{B}}^{+}\right(\mathrm{y}\mathrm{M}\left)\right|\mathrm{B}$

The emf measured is +0.20 V. The cell reaction is

On the basis of electrochemical theory of corrosion, in aqueous solution reaction occuring at the cathode is.

During the electrolysis of fused $\mathrm{NaCl}$, which of these occur at anode?

During electrolysis, the species discharged at the cathode are

When the sample of copper with zinc impurity is to be purified by electrolysis, the appropriate electrodes cathode and anode are respectively? 

 

In a galvanic cell, the electrons flow from