Electrical cells - class-X
| Description: electrical cells | |
| Number of Questions: 21 | |
| Created by: Sundari Chatterjee | |
| Tags: patterns and properties of metals chemistry |
Which of the following statement is incorrect about electrochemical cell?
The following electrochemical cell is taken $Cu| Cu^{2+}(aq)|| Ag^{+}(aq))| Ag$ and has emf $E _{r}>0$ by which of the following actions $E _{1}$ increases?
Find out ${E} _{cell}$ of following electrochemical cell (${E} _{{Br} _{2}/{Br}^{-}}=1.09V$)
$Pt(s)\mid {Br} _{2}(l)\mid{Br}^{-}(0.01M)\mid\mid{H}^{+}(0.01M)\mid{H} _{2}(g)(1bar)\mid Pt(s)$
The following electrochemical cell has been set up: $Pt(s)|Fe^{3+}, Fe^{2+}(a=1)||Ce^{4+}, Ce^{3+}(a=1)|Pt(s); E^{\circ}(Fe^{3+}|Fe^{2+})= 0.77V$; $E^{\circ}(Ce^{4+}|Ce^{3+})= 1.61V$. If an ammeter is connected between the two platinum electrodes, predict the direction of flow of current. Will the current increase or decrease with time?
After some time, the voltage of an electrochemical cell becomes zero. This is because ____________________.
Which one of the following statements is incorrect regarding an electrochemical cell?
The first electro-chemical was invented by:
Statement $1$: In an electrolytic cell, the anode becomes positive and the cathode becomes negative.
Statement $2$: Anions migrate to the anode and cations migrate to the cathode.
The apparatus in which electrical energy is converted into chemical energy is known as:
Consider a spontaneous electrochemical cell containing $Cd, Cd^{2+}, Ag^{+}$, and $Ag$.
The reduction potential of $Cd$ is $-0.403\ V$ and $Ag$ is $0.799\ V$.
Which of the following is true of an electrolytic cell?
The chemical change in an electrolytic cell is non-spontaneous.
What is a voltaic cell?
The value of equilibrium constant for a feasible cell reaction is:
An electrochemical cell consists of?
Consider the reaction;
$Cl _2(g)+2Br^-(aq)\rightarrow 2Cl^-(aq)+Br _2$
The emf of the cell when
$[Cl^-]=[Br _2]=[Br]=0.01 M$ and $Cl _2$ gas at 1 atm pressure will be: ($E^0$ for the above reaction is = 0.29 volt)
In an electrochemical cell, anode and cathode are__________.
Electrochemical cells are also called:
Foe the electrochemical cell:
$Zn\left( s \right) |{ Zn }^{ 2+ }\left( aq \right) \parallel { Cl }^{ - }\left( aq \right) |{ Cl } _{ 2 }\left( g \right) |Pt\left( s \right) $
Given : ${ E } _{ { Zn }^{ 2+ }/Zn }^{ o }=-0.76\ Volt$
${ E } _{ { Cl }^{ - }/{ Cl } _{ 2 }\left( g \right) }^{ o }=-1.36\ Volt$
From these data one can deduce that:
In an electrolytic cell:
The electrochemical cell shown below is a concentration cell.
$M|{ M }^{ 2+ }$ (saturated solution of a sparingly soluble salt, $M{X} _{2})\parallel {M}^{2+}(0.001 mol{dm}^{-3})| M$.
The emf of the cell depends on the difference in concentrations of ${M}^{2+}$ ions at the two electrodes.
The emf of the cell at $298K$ is $0.099V$
The solubility product (${K} _{sp}:{mol}^{3}{dm}^{-9}$) of ${MX} _{2}$ at $298K$ based on the information available for the given concentration cell is: (take $2.303\times R\times 298/F=0.059V$)