Electrochemical Cells

The following electrochemical cell has been set up.

$\begin{array}{l}\mathrm{Pt}\left(1\right)|{\mathrm{Fe}}^{3+},{\mathrm{Fe}}^{2+}(\mathrm{a}=1)||{\mathrm{Ce}}^{4+},{\mathrm{Ce}}^{3+}(\mathrm{a}=1\left)\right|\mathrm{Pt}\left(2\right)\\ \mathrm{E}°({\mathrm{Fe}}^{3+},{\mathrm{Fe}}^{2+})=0.77\mathrm{V}:\mathrm{E}°({\mathrm{Ce}}^{4+},{\mathrm{Ce}}^{3+})=1.61\mathrm{V}\end{array}$
If an ammeter is connected between the two platinum electrodes, predict the direction of flow of current.

How many grams of silver could be plated out on a serving tray by electrolysis of a solution containing silver in +1 oxidation state for a period of 1.0 hours at a current of 8.46 amperes? What is the area of the tray if the thickness of the silver plating is 0.00254 cm? Density of silver is $10.5gc{m}^{-3}.$

The device which convert the energy of combustion of fuels directly into electrical energy is called

The following reaction takes place at $298 \mathrm{K}$ in an electrochemical cell involving two metals $\mathrm{A}$ and $\mathrm{B}$,

${\mathrm{A}}^{2+}\left(\mathrm{aq}\right)+\mathrm{B}\left(\mathrm{s}\right)\to {\mathrm{B}}^{2+}\left(\mathrm{aq}\right)+\mathrm{A}\left(\mathrm{s}\right)$

with $\left[{\mathrm{A}}^{2+}\right]=4\times {10}^{-3} \mathrm{M}$ and $\left[{\mathrm{B}}^{2+}\right]=2\times {10}^{-3} \mathrm{M}$ in the respective half-cells, the cell EMF is $1.091 \mathrm{V}$. The equilibrium constant of the reaction is closest to;

A saturated solution of ${\mathrm{KNO}}_3$ with agar-agar is used to make a 'salt-bridge' because:

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 false?
 

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

What will be at anode and cathode respectively in a Daniell cell? 

A half cell is connected with SHE, during the course of reaction $\mathrm{pH}$ of SHE is increased. The connected half cell behaves as

In the cell represented ${\mathrm{Pb}}_{\left(\mathrm{s}\right)}\left|{\mathrm{Pb}}_{\left(1\mathrm{M}\right)}^{2+}\right|\left|{\mathrm{Ag}}_{\left(1\mathrm{M}\right)}^{+}\right|{\mathrm{Ag}}_{\left(\mathrm{s}\right)}$, the reducing agent is

A variable, opposite external potential $\left({\mathrm{E}}_{\mathrm{e}\mathrm{x}\mathrm{t}}\right)$ is applied to the cell $\mathrm{Z}\mathrm{n}\mathrm{ }|\mathrm{ }\mathrm{Z}{\mathrm{n}}^{2+}\mathrm{ }\left(1\mathrm{M}\right)\parallel \mathrm{C}{\mathrm{u}}^{2+}\mathrm{ }\left(1\mathrm{ }\mathrm{M}\right)|\mathrm{}\mathrm{}\mathrm{C}\mathrm{u}$ , of potential 1.1 V. When ${\mathrm{E}}_{\mathrm{e}\mathrm{x}\mathrm{t}}<1.1\mathrm{ }\mathrm{V}$ and ${\mathrm{E}}_{\mathrm{e}\mathrm{x}\mathrm{t}}>1.1\mathrm{ }\mathrm{V}$ , respectively electrons will flow from:

Two half cells have reduction potentials $–0.76\mathrm{ }\mathrm{V}$ and $–\mathrm{ }0.13\mathrm{ }\mathrm{V}$ respectively. A galvanic cell is made from these two half cells. Which of the following statement is correct?

In which of the following electrochemical cell the overall cell reaction is :

$\mathrm{Z}\mathrm{n}\left(\mathrm{s}\right)+{\mathrm{H}}_2{\mathrm{S}\mathrm{O}}_4\mathrm{ }\left(\mathrm{a}\mathrm{q}\right)\to \mathrm{ }{\mathrm{Z}\mathrm{n}\mathrm{S}\mathrm{O}}_4\mathrm{ }\left(\mathrm{a}\mathrm{q}\right)+{\mathrm{H}}_2\mathrm{ }\left(\mathrm{g}\right)$

In which of the following electrochemical cell overall cell reaction is :

$\mathrm{H}\mathrm{g}\mathrm{O}\mathrm{ }\left(\mathrm{s}\right)+{\mathrm{H}}_2\mathrm{ }\left(\mathrm{g}\right)\to \mathrm{ }\mathrm{H}\mathrm{g}\mathrm{ }\left(\mathcal{l}\right)+{\mathrm{H}}_2\mathrm{O}\mathrm{ }\left(\mathcal{l}\right)$

In which of the following cells net cell reaction is :

${\mathrm{A}\mathrm{g}}^{+}\mathrm{ }\left(\mathrm{a}\mathrm{q}\right)+{\mathrm{C}\mathrm{l}}^{–}\mathrm{ }\left(\mathrm{a}\mathrm{q}\right)\to \mathrm{ }\mathrm{A}\mathrm{g}\mathrm{C}\mathrm{l}\mathrm{ }\left(\mathrm{s}\right)$

In which of the following electrochemical cell overall cell reaction is :

$\mathrm{HgO}\left(\mathrm{s}\right)+{\mathrm{H}}_2\left(\mathrm{g}\right)\to \mathrm{Hg}\left(\mathrm{l}\right)+{\mathrm{H}}_2\mathrm{O}\left(\mathrm{l}\right)$

If a salt bridge is removed from the two half cells, the voltage

In a galvanic cell, the electrons flow from